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3 years ago

1. If we used 0.0100 moles of K2CO3, how many moles of SrCO3 can be expected to form?

Chemistry

1 answer:

faltersainse [42]3 years ago

3 0

Answer:

0.01 moles of SrCO₃

Explanation:

In this excersise we need to propose the reaction:

K₂CO₃ + Sr(NO₃)₂ → 2KNO₃ + SrCO₃

As we only have data about the potassium carbonate we assume the strontium nitrite as the excess reactant.

1 mol of K₂CO₃ react to 1 mol of Sr(NO₃)₂ in order to produce 2 moles of potassium nitrite and 1 mol of strontium carbonate.

Ratio is 1:1. In conclussion,

0.01 mol of K₂CO₃ must produce 0.01 moles of SrCO₃

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Calculate the molecular formula of a compound with the empirical formula C5H11 and a molar mass of 142.32 grams/mole

MA_775_DIABLO [31]

Relative formula mass C₅H₁₁ = 71

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3 years ago

- Standard state refers to

yulyashka [42]

Answer: The standard state refers to 1 atm and $25^{o}C$ .

Explanation:

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So, when the phase of a substance like solid, liquid or gas is present at 1 atmosphere pressure and at a temperature of $25^{o}C$ then it known as standard state of substance.

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2 years ago

The solubility table helps predict the products of what kind of reactions?

Ganezh [65]

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Explanation:

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2 years ago

A sample of nitrogen gas occupies a volume of 2.55 L when it is at 755 mm Hg and 23 degrees Celsius. Use this information to det

ivolga24 [154]

<u>Answer:</u> The number of moles of nitrogen gas are 0.1043 moles and the pressure when volume and temperature has changed is 461.6 mmHg

<u>Explanation:</u>

To calculate the amount of nitrogen gas, we use the equation given by ideal gas which follows:

$PV=nRT$

where,

P = pressure of the gas = 755 mmHg

V = Volume of the gas = 2.55 L

T = Temperature of the gas = $23^oC=[23+273]K=296K$

R = Gas constant = $62.364\text{ L.mmHg }mol^{-1}K^{-1}$

n = number of moles of nitrogen gas = ?

Putting values in above equation, we get:

$755mmHg\times 2.55L=n\times 62.364\text{ L.mmHg }mol^{-1}K^{-1}\times 296K\\\\n=\frac{755\times 2.55}{62.364\times 296}=0.1043mol$

To calculate the pressure when temperature and volume has changed, we use the equation given by combined gas law.

The equation follows:

$\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}$

where,

$P_1,V_1\text{ and }T_1$ are the initial pressure, volume and temperature of the gas

$P_2,V_2\text{ and }T_2$ are the final pressure, volume and temperature of the gas

We are given:

$P_1=755mmHg\\V_1=2.55mL\\T_1=23^oC=[23+273]K=296K\\P_2=?\\V_2=4.10L\\T_2=18^oC=[18+273]K=291K$

Putting values in above equation, we get:

$\frac{755mmHg\times 2.55L}{296K}=\frac{P_2\times 4.10L}{291K}\\\\P_2=\frac{755\times 2.55\times 291}{4.10\times 296}=461.6mmHg$

Hence, the number of moles of nitrogen gas are 0.1043 moles and the pressure when volume and temperature has changed is 461.6 mmHg

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3 years ago

Read 2 more answers

Compounds put together will form -

Paraphin [41]

The correct answer is B. Compounds put together will form mixtures because compounds itself are pure substances which contains elements and atoms. Mixtures is a system that is made up of two or more substances or compounds which are not combined chemically.

4 0

3 years ago

1. If we used 0.0100 moles of K2CO3, how many moles of SrCO3 can be expected to form?​

1. If we used 0.0100 moles of K2CO3, how many moles of SrCO3 can be expected to form?