The question is incomplete. The complete question is :
Acetylene 
gas is often used in welding torches because of the very high heat produced when it reacts with oxygen 
gas, producing carbon dioxide gas and water vapor. Calculate the moles of oxygen needed to produce 1.5 mol of carbon dioxide. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits.
Answer: 1.9 moles of oxygen are needed to produce 1.5 moles of carbon dioxide.
Explanation:
According to the law of conservation of mass, mass can neither be created nor be destroyed. Thus the mass of products has to be equal to the mass of reactants. The number of atoms of each element has to be same on reactant and product side. Thus chemical equations are balanced.
The balanced reaction for combustion of acetylene is:
According to stoichiometry;
4 moles of carbon dioxide are produced by = 5 moles of oxygen
Thus 1.5 moles of carbon dioxide are produced by =
moles of oxygen
Thus 1.9 moles of oxygen are needed to produce 1.5 moles of carbon dioxide.
The person drinks 328500 ml or 328.5 liters of water in a year.
Answer:
4.5g/ml
Explanation:
metal sample has a mass = 7.56 g
cylinder previously filled with water = 20.00 mL
final volume in the cylinder = 21.68 mL
density = 4.5g/ml
Squeezing just the juices out of the orange, like with your hand or whatever you use, is a physical change. yes :)
<u>Answer:</u> The equilibrium constant for the given reaction is 1.33
<u>Explanation:</u>
We are given:
Equilibrium concentration of ammonia = 2 M
Equilibrium concentration of nitrogen gas = 3 M
Equilibrium concentration of hydrogen gas = 1 M
For the given chemical equation:
The expression of 
for above equation follows:
![K_{eq}=\frac{[NH_3]^2}{[N_2][H_3]^3}](https://tex.z-dn.net/?f=K_%7Beq%7D%3D%5Cfrac%7B%5BNH_3%5D%5E2%7D%7B%5BN_2%5D%5BH_3%5D%5E3%7D)
Putting values in above equation, we get:
Hence, the equilibrium constant for the given reaction is 1.33
