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13 Dec 2019

If a 8.55 mil of C5H12 reacts with excess O2 how many moles of CO2 will be produced in the following reaction

C5H12+8O2 yields 6H2O+5CO2

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Reid Wolff
Reid WolffLv2
17 Dec 2019

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Related questions

Consider the following unbalanced chemical equation for the combustion of pentane C5H12

C5H12 (l) O2 (g)  CO2 (g) H2O (l) 

If 20.4 g of pentane are burned in excess oxygen, what mass of water can be produced, assuming 100% yield?

1.A system releases 691 kJ of heat and does 100 kJ of work on the surroundings.

What is the change in internal energy of the system? Express your answer to 2 sig figs.

2.If 1.7 g of matter were converted to energy, how much energy would be formed?

Express your answer using two significant figures.

3.Hydrogen gas reacts with oxygen to form water.

2H2(g)+O2(g)→2H2O(g)ΔH=−483.5kJ

Determine the minimum mass of hydrogen gas required to produce 524 kJ of heat.

Express your answer to three significant figures and include the appropriate units.

4. Calculate ΔHrxn for the following reaction:
5C(s)+6H2(g)→C5H12(l)
Use the following reactions and given ΔH′s.
C5H12(l)+8O2(g)→5CO2(g)+6H2O(g), ΔH= -3244.8 kJ
C(s)+O2(g)→CO2(g), ΔH= -393.5 kJ
2H2(g)+O2(g)→2H2O(g), ΔH= -483.5 kJ

Express answer to 4 sig figs.

5.

Use the ΔH°f and ΔH°rxn information provided to calculate ΔH°f for IF:

ΔH°f (kJ/mol) IF7(g) + I2(g) → IF5(g) + 2 IF(g) ΔH°rxn = -89 kJ
IF7(g) -941
IF5(g) -840
a.101 kJ/mol
b.-146 kJ/mol
c. -190 kJ/mol
d. -95 kJ/mol
e. 24 kJ/mol

Consider the following reaction. C5H12(g) + 8 O2(g) → 5 CO2(g) + 6 H2O(g) If a container were to have 28 molecules of C5H12 and 28 molecules of O2 initially, how many total molecules (reactants plus products) would be present in the container after this reaction goes to completion? (Use only whole numbers to solve.)

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