How much Bicarbonate of Soda and Vinegar would I need to reach space? So here is my problem - as part of my job I present some science demonstrations to children and one of the tricks I regularly use is the bicarb/acetic acid rocket. I thought the other day that a really fun fact to give them to go along with it would be the amount of bicarb and vinegar you would need to, say, escape the Earth's atmosphere. I'm a bit rusty but I think it's less trivial than it sounds. I think you need the rocket equation, which means you need the exhaust velocity, which is in turn quite complex to calculate. Does anyone have any simpler approaches which might work? 
A few nuggets which might help: 
1 mole of bicarb produces 291 cc of CO2. 
Escape velocity is ~11000 m/s
Any answers will be very appreciated! 
 A: rocket fuel is often characterised by its Specific Impulse.  Loosely this is a measure of force applied to rocket per mass of fuel.  I'm afriad I don't know what this would be for Bicarb...
A: When you say "reach space" do you mean a) get above most of the atmosphere, b) achieve orbit velocity, or c) achieve earth escape velocity?
Either way, if you simplify the problem by ignoring air friction, it's only a matter of achieving a certain velocity.
Robert H. Goddard showed that, if you built your rocket a certain way, you could achieve any desired velocity. (I'm very much simplifying and paraphrasing.)
Suppose you wish to accelerate 1 mass unit to velocity $v$.
Assume you do this by making a rocket consisting of $M$ mass units, which is all fuel except for the 1 mass unit left at the end.
Then the total mass you need is $M = e^{v/c}$, where $c$ is the velocity of the exhaust.
That means, for example, if you double $v$ you have to square $M$, but if you can double the exhaust velocity $c$, you can reduce $M$ to its square root.
That's why exhaust velocity is so important.
This does require that the fuel container not only be as light as possible, but it should fall away as the fuel burns.
That's why space rockets have multiple stages.
ADDED: Some common exhaust velocities, taken from Goddard's paper, are:
- Common black-powder rocket: 29 m/s
- "Coston" ship rocket: 31 m/s
He found that by carefully building a rocket chamber and exhaust nozzle, he could get up to exhaust velocities of over 2,400 m/s using special gunpowder.
That's a factor of 80, meaning M could be reduced by a power of 80.
The specific impulse of $H_2$ is up around 5000 seconds more or less, times $g$ of $10ms^{-2}$ or 50000 m/s, 20 times faster than the gunpowder, so an additional power of 20 reduction.
A: I also was wondering this, and since there was no answer I did the best I could.
We need to know the specific impulse of vinegar and baking soda, and to do that we need to know the chemical potential energy and molar mass of the fuel.
Vinegar and baking soda cause an endothermic reaction, so we need to find the Gibb's Free Energy $\triangle G$, which is the change in enthalpy (of the products vs the inputs) $\triangle H$ minus the change in entropy $\triangle S$, times the temperature $T$. These values can vary based on many factors but you can look up the "standard" values for a rough estimate.
Following the approximate chemical equation:
$NaHCO^3 + HC^2H^3O^2 → H^2O + CO^2 + Na^+ + CH^2COO^-$
We can find the enthalpy of and entropy for each:




Chemical
Enthalpy
Entropy
Molar mass




Na+
-240 kJ/mol
59 J / mol K
22 g/mol


CH3COO-
-486 kJ/mol
86 J / mol K
59 g/mol


H2O
-285 kJ/mol
70 J / mol K
18 g/mol


CO2
-393 kJ/mol
213 J / mol K
44 g/mol


NaHCO3
-950 kJ/mol
101 J / mol K
84 g/mol


HC2H3O2
-483 kJ/mol
158 J / mol K
60 g/mol


All Products
-1404 kJ/mol
421 J / mol K
143 g/mol


All Inputs
-1433 kJ/mol
259 J / mol K
143 g/mol




So to find the Gibb's Free Energy, we use $\triangle G = \triangle H - T \triangle S$ at 298K which is $ \triangle G = -19kJ$. Negative indicates a spontaneous reaction, and energy that went somewhere else during the reaction. Also note that entropy is in joules and enthalpy is in kilojoules, so be sure to convert otherwise you will get a wildly wrong answer.
Now that we know this excess energy, we can get a best case scenario where all of that energy goes into accelerating all of the products using $KE = 1/2mv^2$, which we can reformulate as $v = \sqrt(2KE / m)$.
We are assuming $KE = 19kJ$, but we also must know the mass of the products. If we were just reacting sodium bicarbonate with acetic acid, that would be .143kg, with a resulting $v = 515m/s$. However, we must remember that the vinegar in our rocket is 95% water, so our product mass is 1.5kg, and $v = 159m/s$.
With this velocity we can simply divide by $G$ to get a pitiful specific impulse of $16m/s$, and we are ready to apply the rocket equation.
In theory any amount of baking soda and vinegar could be enough to take you to space, as long as you had a light enough vehicle. So what the rocket equation will tell us is the percentage of a rocket that must be fuel to achieve a certain speed based on this specific impulse, assuming no losses to drag etc.
$\triangle v = I_{sp}g_0\ln(m_0/m_f)$
If we want to reach an orbital velocity of 7660m/s (the velocity of the ISS),  we must have 10^21 as much fuel as we have payload. That's a fuel:payload ratio of one septillion to one.
If we're solving the obvious problem of how vinegar is 95% water, we can do much better, with a fuel:payload ratio of merely 5.5 million to one. Seeing as the smallest dry mass rocket ever to reach orbit weight about 600kg, that would imply a craft with perhaps 3.3 million metric tons of sodium bicarbonate and acetic acid fuel -- weighing the same as about one thousand saturn V rockets.
So in summary, if you have a ten year old you are teaching who weighs 30kg, and asks you how much baking soda and vinegar it would take to reach space, the answer is that they would need 30 septillion kg of vinegar and baking soda to for them to reach orbit -- and that's with impossibly perfect engineering. But if you loosen the constraints it maybe just maybe would only take a rocket 1000x bigger than the biggest rocket ever created.
