Home > Chemistry > Stoichiometry

What is the mass of water produced when 9.33 g of butane reacts with excess oxygen?

Answer 1

Serenity Allen

#5xx0.161*molxx18.01*g*mol^-1=??#

#C_4H_10(g) + 13/2O_2(g) rarr 4CO_2(g) + 5H_2O(l)#

#"Moles of butane"# #=# #(9.33*g)/(58.12*g*mol^-1)# #=# #0.161*mol#.

Assuming total combustion, we know that butane burns completely to release five mol of water per mole.

Given that we know the molar quantity of butane, we simply perform the operation, #5xx0.161*molxx18.01*g*mol^-1=??#

How much carbon dioxide gas has evolved during the reaction in terms of mass?

By signing up, you agree to our Terms of Service and Privacy Policy

Answer 2

Wyatt Atkins

To determine the mass of water produced, you first need to balance the chemical equation for the combustion of butane. Then, you can use stoichiometry to find the mass of water produced.

By signing up, you agree to our Terms of Service and Privacy Policy

Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.