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2 years ago

What volume will 35.9 g of hydrogen gas (H2) occupy at STP?

Chemistry

2 answers:

Nataly [62]2 years ago

8 0

35.9g x 1 mol/ 2.016g x 22.4 L/ 1 mol= 398.89 L

notka56 [123]2 years ago

6 0

Answer: 402.08 L

Explanation: According to avogadro's law, 1 mole of every substance occupies 22.4 Liters at STP and contains avogadro's number $6.023\times 10^{23}$ of particles.

To calculate the moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text {Molar mass}}$

$\text{Number of moles}=\frac{35.9 g}{2g/mol}=17.95moles$

Now 1 mole of $H_2$ molecule occupy= 22.4 L at STP

17.95 moles of $H_2$ molecule contains = $\frac{22.4}{1}\times 17.95=402.08 L$ at STP

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In a reaction of a potential new fuel, it is found that when 2.81 moles of the fuel combusts, 1,612 kJ of energy is released. Wh

Tema [17]

Answer:

-573.67

Explanation:

whenever energy is released in a chemical reaction, we would then expect the delta H of the reaction to be negative because the reaction is an exothermic reaction.

now we have that 2.81 moles of fuel when it combusts would releases 1612kJ of energy

thus, 1 mole will release 1612/2.81 = -573.67kJ of heat

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3 0

2 years ago

Use the law of conservation of mass to answer the questions. Consider a hypothetical reaction in which A and B are reactants and

shutvik [7]

Answer:

26 grams of D will be produced.

Explanation:

The reaction is given by:

A + B -----> C + D

Mass of A reacted = 21 g

Mass of B reacted = 22 g

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Mass of D formed = m =?

According to law of conservation of mass, the total mass of the reactants used is equal to the total mass of the product formed.

Then:

mass of A reacted + mass of B reacted = mass of C formed + mass of D formed

21 + 22 = 17 + m

m = 26 g

5 0

3 years ago

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zalisa [80]

Answer:

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Explanation:

8 0

3 years ago

Calculate the molar solubility of CaF2 at 25°C in a solution that is 0.010 M in Ca(NO3)2. The Ksp for CaF2 is 3.9 x 10-11.

madreJ [45]

Answer:

$Molar \ solubility=3.12x10^{-5}M$

Explanation:

Hello,

In this case, for the dissociation of calcium fluoride:

$CaF_2(s)\rightleftharpoons Ca^{2+}+2F^-$

The equilibrium expression is:

$Ksp=[Ca^{2+}][F^-]^2$

In such a way, via the ICE procedure, including an initial concentration of calcium of 0.01 M (due to the calcium nitrate solution), the reaction extent $x$ is computed as follows:

$3.9x10^{-11}=(0.01+x)(2*x)^2\\\\x=0.0000312M$

Thus, the molar solubility equals the reaction extent $x$ , therefore:

$Molar \ solubility=3.12x10^{-5}M$

Regards.

4 0

3 years ago

The decomposition of SOCl2 is first-order in SOCl2. If the half-life for the reaction is 4.1 hr, how long would it take for the

qaws [65]

4.1 h = 14760 s

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k = rate reaction = 4.97 x 10^-5 

ln 0.045 / 0.36 = - 4.97 x 10^-5 t 

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t = 41839.9 s = 11 h 37 min 19 s

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3 years ago