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2 years ago

What mass of carbon monoxide must be burned to produce 175 kj of heat under standard state conditions?

Chemistry

2 answers:

Soloha48 [4]2 years ago

8 0

When 2.50 g is burned then in oxygen then 1.25kj of heat is produced.

Mrrafil [7]2 years ago

7 0

Answer:

17.3 g

Explanation:

Let's consider the combustion of CO.

CO(g) + 0.5 O₂(g) → CO₂(g)

We can find the standard enthalpy of the reaction using the following expression.

ΔH°rxn = 1 mol × ΔH°f(CO₂(g)) - 1 mol × ΔH°f(CO(g)) - 0.5 mol × ΔH°f(O₂(g))

ΔH°rxn = 1 mol × (-393.5 kJ/mol) - 1 mol × (-110.5 kJ/mol) - 0.5 mol × 0

ΔH°rxn = -283.0 kJ

283.0 kJ are released per mole of CO. The moles of CO required to release 175 kJ are:

(-175 kJ) × (1 mol CO/ -283.0 kJ) = 0.618 mol CO

The molar mass of CO is 28.01 g/mol. The mass of CO is:

0.618 mol × (28.01 g/mol) = 17.3 g

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A solution prepared by mixing 10 ml of 1 m hcl and 10 ml of 1.2 m naoh has a ph of

blagie [28]

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Explanation:

pH is the measure of acidity or alkalinity of a solution.

Moles of $H^+$ ion = $Molarity\times {\text {Volume in L}}=1M\times 0.01L=0.01mol$

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For neutralization:

1 mole of $H^+$ ion will react with 1 mole of $OH^-$ ion

0.01 mol of $H^+$ ion will react with = $\frac{1}{1}\times 0.01mole$ of $OH^-$ ion

Thus (0.012-0.01)= 0.002 moles of $OH^-$ are left in 20 ml or 0.02 L of solution.

$[OH^-]=\frac{0.002}{0.02L}=0.1M$

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$pOH=-log[0.1]=1$

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