Fe + O2 à Fe2O3 1. How many moles of iron (lll) oxide are produced from 0.275 moles of diatomic oxygen?

2. How many moles of iron are required to react with 0.275 moles of diatomic oxygen?

C4H10 + O2 à CO2 + H2O

3. How many grams of butane (C4H10) are required to burn 3.63 moles of oxygen?

4. How many moles of carbon dioxide are produced if 9.45 moles of water are also produced?

5. How many moles of butane are required to react with 0.25 moles of oxygen?

6. How many grams of oxygen are required to produce 13.9 g of carbon dioxide?

when 25.0 ml of 0.700 mol/l naoh was mixed in a calorimeter with 25.0 ml of 0.700 mol/l hcl, both initially at 20.0 °c, the temperature increased to 22.1 °c. the heat capacity of the calorimeter is 279 j/°c.

the equation for the reaction is:

naoh + hcl → nacl + h₂o

moles of hcl = 0.0250 l hcl ×

0.700

mol hcl

1 l hcl = 0.0175 mol hcl

volume of solution = (25.0 + 25.0) ml = 50.0 ml

mass of solution = 50.0 ml soln ×

1.00

ml soln

= 50.0 g soln

δt=t2-t1

= (22.1 – 20.0) °c = 2.1 °c

the heats involved are

heat from neutralization + heat to warm solution + heat to warm calorimeter = 0

q1+q2+q3=0

nδh+mcδt+cδt=0

0.0175 mol ×

δh

+ 50.0 g × 4.184 j·g⁻¹°c⁻¹ × 2.1 °c + 279 j°c⁻¹ × 2.1 °c = 0

0.0175 mol ×

δh

+ 439.32 j + 585.9 j = 0

0.0175 mol ×

δh

= -1025.22 j

δh=1025.22j0.0175 mol= -58 600 j/mol = -58.6 kj/mol

with this one i know the answer in craters one reason i looked it up and i learned about it there is my evidence

you need to have a picture of the atom that way we can answer it