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3 years ago

4Cuo - 2Cu,O + O, AH = 288 kJ

Chemistry

1 answer:

Anna35 [415]3 years ago

6 0

I am a little slow i cannot help with these that why i got this app lol

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Gaseous compound Q contains only xenon and oxygen. When 0.100 gg of Q is placed in a 50.0 mLmL steel vessel at 0 ∘C∘C, the press

asambeis [7]

The question is incomplete, here is the complete question:

Gaseous compound Q contains only xenon and oxygen. When a 0.100 g sample of Q is placed in a 50.0-mL steel vessel at 0°C, the pressure is 0.229 atm. What is the likely formula of the compound?

A. XeO

B. $XeO_4$

C. $Xe_2O_2$

D. $Xe_2O_3$

E. $Xe_3O_2$

<u>Answer:</u> The chemical formula of the compound is $XeO_4$

<u>Explanation:</u>

To calculate the molecular mass of the compound, we use the equation given by ideal gas equation:

PV = nRT

Or,

$PV=\frac{w}{M}RT$

where,

P = Pressure of the gas = 0.229 atm

V = Volume of the gas = 50.0 mL = 0.050 L (Conversion factor: 1 L = 1000 mL)

w = Weight of the gas = 0.100 g

M = Molar mass of gas = ?

R = Gas constant = $0.0821\text{ L atm }mol^{-1}K^{-1}$

T = Temperature of the gas = $0^oC=273K$

Putting value in above equation, we get:

$0.229\times 0.050=\frac{0.100}{M}\times 0.0821\times 273\\\\M=\frac{0.100\times 0.0821\times 273}{0.229\times 0.050}=195.4g/mol\approx 195g/mol$

The compound having mass as 195 g/mol is $XeO_4$

Hence, the chemical formula of the compound is $XeO_4$

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3 years ago

What must be known for the rate constant to be calculated from the rate law?

joja [24]

Answer:

C. The reaction rate at known reaction concentrations

Explanation:

The rate of a reaction is the measure of the speed of a chemical reaction. To find the rate constant of a reaction, the concentration of the reactants must be known.

Reaction rate is directly proportional to the concentration of the reactants.
The quantitative relationship between the rate of a reaction and the concentrations of reactants is expressed as the rate law.
From this we can deduce the rate constant.

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sleet_krkn [62]

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what is the balanced equation of magnesium carbonate decomposes on heating to form magnesium oxide and carbon dioxide

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Answer:

ExplaAt high temperatures MgCO3 decomposes to magnesium oxide and carbon dioxide. This process is important in the production of magnesium oxide. This process is called calcining: MgCO3 → MgO + CO2 (ΔH = +118 kJ/mol)

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Oxygen and hydrogen are both elements that are found as gases at room temperature. When oxygen combines with hydrogen, they prod

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Answer:

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has properties that are different from the original substances.

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