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MaRussiya [10]
3 years ago
5

A balloon of helium was put in the freezer at -23°C. Its volume at this temperature was 2.5 liters. It was removed from the free

zer. Eventually, it reached a temperature of 177°C. What would its volume be at this temperature? (Neglect any force used to stretch the rubber balloon.) (1.)45000 (2.) 0.22 (3.) 4.5 (4.) 1.4
Chemistry
1 answer:
kotegsom [21]3 years ago
3 0

4.5 L

Explanation:

We will use the combined gas law formula;

P₁V₁/T₁ = P₂V₂/T₂

Because the pressure remains the same, it cancels out and what remains is;

V₁/T₁ = V₂/T₂

Before evaluating remember to change the temperatures into Kelvin;

-23° = 250.15 K

177° = 450.15 K

We replace the variables with known values;

2.5 / 250.15 = V₂ / 450.15

V₂ = 2.5 /250.15 * 450.15

V₂ = 4.4988 L

≅ 4.5 L

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When 6.13 g of a certain molecular compound X are dissolved in 90. g of formamide (NH2COH), the freezing point of the solution i
belka [17]

Answer:

321.6 g/Mol

Explanation:

mass of solvent in kilograms = 90g/1000 = 0.09 Kg

Given that;

ΔTf = Kf . m . i

Where;

Kf = freezing point constant = 4.25 °C/Kg mol

m = molality of the solution

i = Van't Hoff factor = 1 (since the substance is molecular)

ΔTf = freezing point of pure solvent - freezing point of solution

freezing point of pure solvent = 3 °C

ΔTf = 3 °C - 2.1 °C

ΔTf = 0.9  °C

0.9= 4.25 * 6.13/M/0.09 * 1

0.9= 26.0525/M * 1/0.09

0.9 = 26.0525/0.09 M

0.9 * 0.09M = 26.0525

M = 26.0525/0.9 * 0.09

M= 321.6 g/Mol

8 0
3 years ago
If 10 grams of potassium chlorate decompose to form potassium chloride and oxygen gas inside a 500 mL container at a temperature
Gekata [30.6K]

Answer:

10 atm

Explanation:

There's a lot to do here, but lets take it one step at a time. First, let's write a balanced equation for the decomposition of potassium chlorate into potassium chloride and oxgyen gas.

2 KClO3 → 2 KCl + 3 O2

Now let's find the moles of the KClO3 (molar mass 122.55 g/mol) that we have take 10 g/122.55 g/mol, grams will cancel and we are left with 0.0816 moles. lets divide that by two since we have a two in front of the KClO3 in the equation, and then multiply that number by 5 since it's the total moles of products, in summary, multiply by 5/2 to get 0.204 moles.

Now that we know the moles of our products, let's plug some stuff into the ideal gas law PV = nRT. We are looking for P so let's solve for that. P = (nRT)/V, now let's plug in our values. Make sure V is converted to liters so 0.5 L. And convert celcius to kelvin by adding 273

P = ((0.204 moles)(318 K)(0.08206 L atm mol^-1 K^-1))/0.5 L

A lot of units cancel, and we get about 10.65 atm, if you don't want the answer in atm, you can find a conversion equation. But let's round to sig figs for now, which will bring us to 10 atm.

3 0
2 years ago
What volume of a 6.0m hcl solution is required to make 250.0 milliters of 1.5 m hcl
Georgia [21]

Answer : The volume for 6.0m HCl solution required = 62.5 ml

Solution : Given,

Initial concentration of HCl solution = 6.0m

Final concentration of HCl solution = 1.5m

Final volume of HCl solution = 250 ml

Initial volume of HCl solution = ?

Formula used for dilution is,

M_1V_1=M_2V_2

where,

M_1 = initial concentration

M_2 = final concentration

V_1 = initial volume

V_2 = final volume

Now put all the given values in above formula, we get the initial volume of HCl solution.

6.0m\times V_1=1.5m\times 250ml

V_1 = 62.5 ml

Therefore, the volume for 6.0m HCl solution required = 62.5 ml


8 0
3 years ago
Show all calulations
Black_prince [1.1K]
Im confused here. Add the rest of the question for me to help you
5 0
2 years ago
What test was used to identify hydrogen gas? Write a balanced equation to represent the test?
const2013 [10]
Burning splint test
2H2 (g) + O2 (g) -> 2H20 (g) + heat
It’s a combustion reaction
6 0
3 years ago
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