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Mama L [17]
2 years ago
11

what is the limiting reactant of 20.0 moles of o2 react with 30.0 moles of h2 according to the following reaction ? 2H2 + O2 = 2

H2O
Chemistry
1 answer:
IRINA_888 [86]2 years ago
5 0

Answer:

The limiting reactant is hydrogen.

Explanation:

According to the balanced equation for synthesis of water, hydrogen is used up twice as fast as oxygen -- we need two moles of H2 for every one mole of O2 when creating water.

Since we have 20 moles of oxygen, this means we would need twice as much hydrogen, or 40 moles, to use it all up. There is only 30 moles of hydrogen, which means that all the hydrogen will be used before the 20 moles of oxygen is used. Hydrogen limits production in this case.

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The volume of a gas is 27.5 mL at 22.0°C and 0.974 atm. What will the volume be at 15.0°C and 0.993 atm? Use Ideal Gas Law (PV =
Scorpion4ik [409]

Answer:

26.3 mL

Explanation:

Step 1:

Obtaining an appropriate gas law from the ideal gas equation.

This is illustrated below:

From the ideal gas equation:

PV = nRT

Divide both side by T

PV/T = nR

At this stage, we'll assume the number of mole (n) to be constant.

Note: R is the gas constant.

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We can thus, write the above equation as:

P1V1/T1 = P2V2/T2

The above equation is called the general gas equation.

Step 2:

Data obtained from the question. This includes the following:

Initial volume (V1) = 27.5 mL

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Initial pressure (P1) = 0.974 atm.

Final temperature (T2) = 15.0°C = 15.0°C + 273 = 288K

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Step 3:

Determination of the final volume of the gas using the general gas equation obtained. This is illustrated below:

P1V1 /T1 = P2V2/T2

0.974 x 27.5/295 = 0.993 x V2/288

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4 0
2 years ago
Consider the hypothetical atom x. if the molecular formula for lithium carbonate is li2co3 and the formula of x chloride is xcl3
eduard
First step is to determine the valency of each of x and CaCO3 from the given compounds:

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7 0
2 years ago
Zinc has a mass of 4.50g calculate the volume
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Divide the mass by the density

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An evaporation–crystallization process of the type described in Example 4.5-2 is used to obtain solid potassium sulfate from an
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\frac{M_{3}}{M_{1}} = 352.5/220.77 = 1.6

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