(Can you please show all the work that was needed for the problems thank youu sm)

15. One of the reactions used to inflate automobile air bags involves
sodium azide (NaN3): 2NaN3(s) —> 2Na(s) + 3N2(g). Determine the
mass of N2 produced from the decomposition of NaN3 shown at right.
16. Challenge in the formation of acid rain, sulfur dioxide (S02) reacts with
oxygen and water in the air to form sulfuric acid (H2SO4) Write the
balanced chemical equation for the reaction. If 2.50 g of SO2 reacts with
excess oxygen and water, how much H2SO4 in grams, is produced?

away from the curb

explanation:

the wheels would then hit the curb if it started to rolling, decreasing the chance of an accident.

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

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