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3 years ago

2) Find the volume that 2.0 moles of H2 will occupy at STP?

Chemistry

1 answer:

Rom4ik [11]3 years ago

4 0

Answer:

V = 44.85 L

Explanation:

Given data:

Volume of H₂ = ?

Number of moles of H₂ = 2.0 mol

Given temperature = 273.15 K

Given pressure = 1 atm

Solution:

Formula:

PV = nRT

P = Pressure

V = volume

n = number of moles

R = general gas constant = 0.0821 atm.L/ mol.K

T = temperature in kelvin

By putting values,

1 atm × V = 2.0 mol × 0.0821 atm.L/ mol.K × 273.15 K

V = 44.85 atm.L / 1 atm

V = 44.85 L

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Iron(II) can be oxidized by an acidic K2Cr2O7 solution according to the net ionic equation: Cr2O72− + 6Fe2+ + 14H+ → 2Cr3+ + 6Fe

cestrela7 [59]

Answer:

The molar concentration of Fe²⁺ in the original solution is 1.33 molar

Explanation:

Moles of K₂Cr₂O₇ = Molarity x Volume (lit)

= 0.025 x 35.5 x 10⁻³

= 0.0008875

Cr₂O₇²⁻ + 6 Fe²⁺ + 14 H⁺ → 2 Cr³⁺ + 6 Fe³⁺ + 7 H₂O

From equation

1 mole K₂Cr₂O₇ used for the oxidation of 6 moles Fe²

0.0008875 mole K₂Cr₂O₇ used for the oxidation of = $\frac{6 X 0.0008875}{1}$ = 0.005325 mole of Fe²

Molarity = $\frac{No. of moles of solute}{Volume of solution(lit)}$

Molar concentration of Fe² = $\frac{0.005325 X 1000}{25}$ = 1.33 molar

So molar concentration of Fe²⁺ in the original solution = 1.33 molar

4 0

3 years ago

In a student experiment, the empirical formula of a copper halide was found by adding aluminum metal to an aqueous solution of t

Radda [10]

Answer: The empirical formula for the given compound is $CuCl_3$

Explanation:

We are given:

Mass of copper chloride in 1 L or 1000 mL of solution = 42.62 grams

Taking Trial A:

Volume of solution = 49.6 mL

Applying unitary method:

In 1000 mL of solution, the mass of copper chloride present is 42.62 grams

So, in 49.6 mL of solution, the mass of copper chloride will be = $\frac{42.62}{1000}\times 49.6=2.114g$

We are given:

Mass of filter paper = 0.908 g

Mass of filter paper + copper = 1.694 g

Mass of copper = [1.694 - 0.908] g = 0.786 g

Mass of chlorine in the sample = [2.114 - 0.786]g = 1.328 g

To formulate the empirical formula, we need to follow some steps:

Step 1: Converting the given masses into moles.

Moles of Copper = $\frac{\text{Given mass of Copper}}{\text{Molar mass of Copper}}=\frac{0.786g}{63.5g/mole}=0.0124moles$

Moles of Chlorine = $\frac{\text{Given mass of Chlorine}}{\text{Molar mass of Chlorine}}=\frac{1.328g}{35.5g/mole}=0.0374moles$

Step 2: Calculating the mole ratio of the given elements.

For the mole ratio, we divide each value of the moles by the smallest number of moles calculated which is 0.0124 moles.

For Copper = $\frac{0.0124}{0.0124}=1$

For Chlorine = $\frac{0.0374}{0.0124}=3.02\approx 3$

Step 3: Taking the mole ratio as their subscripts.

The ratio of Cu : Cl = 1 : 3

Hence, the empirical formula for the given compound is $CuCl_3$

3 0

3 years ago

Consider the balanced equation below.

Vikki [24]

Answer: The mole ratio of $PCl_3$ to $PCl_5$ is 1: 1

Explanation:

According to the balanced chemical equation ,the number of atoms of each element has to be same on reactant and product side. The stoichiometric coefficients of the species represent their number of moles.

$PCl_3+Cl_2\rightarrow PCl_5$

Thus in the reactants, there is 1 mole of $PCl_3$ and 1 mole of $Cl_2$ molecule. And thus there is 1 mole of $PCl_5$ in the product as well.

Thus the mole ratio of $PCl_3$ to $PCl_5$ is 1: 1

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3 years ago

For questions 14-16 pick out the variables that will be needed to answer the following question: Do trees grow faster if it is w

Sveta_85 [38]

Answer:

14) A. amount of rain

15) C. amount of growth

16) B. no rainfall

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3 years ago

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What type of reaction produces a metal from its metal oxide

Nataly [62]

This is a reduction reaction as the oxide(oxygen) is taken away from the metal =]

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3 years ago