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1 year ago

Can someone put their own numbers in this sentence and solve it? Thanks!

1 answer:

4 0

A balloon with a pressure of 1 atm and a temperature of 17° Celsius has a volume of 1000 mL. The day warms up and increases the temperature to 27° Celsius, which makes the pressure change to 1520 mm Hg.What is the new volume of the balloon, in Liters?

The new volume of the balloon is <u>0.517 L.</u>

By ideal gas law, PV = nRT

P = pressure

V = volume

n = number of mole of gas

R = gas constant

T = temperature

Using ideal gas law, P₁V₁/ T₁ = P₂V₂/ T₂

P₁= 1 atm

V₁ = 1000 mL = 1 L

T₁ = 17° C = 290 K

After the day warms up:-

P₂ = 1520 mm Hg = 2 atm

T₂ = 27° C = 300 K

Put these values in formula, P₁V₁/ T₁ = P₂V₂/ T₂

V₂ = P₁V₁T₂/ T₁ P₂

V₂ = 1 atm× 1 L × 300 K/ 290 K × 2 atm

V₂ = 0.517 L = 517 mL

Hence, the new volume of the balloon is 0.517 L.

The ideal gas equation is formulated as: PV = nRT.

In this equation, P refers to the pressure of the ideal gas, V is the volume of the ideal gas, n is the overall quantity of ideal gas this is measured in terms of moles, R is the universal gas constant, and T is the temperature.

Learn more about ideal gas law here:- brainly.com/question/25290815

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Calculate the molarity of a solution containing 15.2 grams of NaCl dissolved in 2.5 L of solution.

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Answer:

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Explanation:

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3 years ago

what is the chemical reaction in which the exchange of electropositive and electronegative ions occurs in aqueous solution

defon

Answer:

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3 years ago

Read 2 more answers

How many moles of na2co3 are necessary to reach stoichiometric quantities with cacl2

lbvjy [14]

0.0102 moles Na₂CO₃ = 1.08g of Na₂CO₃ is necessary to reach stoichiometric quantities with cacl2.

<h3>Explanation:</h3>

Based on the reaction

CaCl₂ + Na₂CO₃ → 2NaCl + CaCO₃

1 mole of CaCl₂ reacts per mole of Na₂CO₃

we have to calculate how many moles of CaCl2•2H2O are present in 1.50 g

We must calculate the moles of CaCl2•2H2O using its molar mass (147.0146g/mol) in order to answer this issue.
These moles, which are equal to moles of CaCl2 and moles of Na2CO3, are required to obtain stoichiometric amounts.
Then, we must use the molar mass of Na2CO3 (105.99g/mol) to determine the mass:

<h3>Moles CaCl₂.2H₂O:</h3>

1.50g * (1mol / 147.0146g) = 0.0102 moles CaCl₂.2H₂O = 0.0102moles CaCl₂

Moles Na₂CO₃:

0.0102 moles Na₂CO₃

Mass Na₂CO₃:

0.0102 moles * (105.99g / mol) = 1.08g of Na₂CO₃ are present

Therefore, we can conclude that 0.0102 moles Na₂CO₃ is necessary.to reach stoichiometric quantities with cacl2.

To learn more about stoichiometric quantities visit:

<h3>brainly.com/question/28174111</h3>

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7 0

2 years ago

Please help me, I really don't want to fail but I don't know how to do this

Brrunno [24]

Answer:

<u>12 moles</u>

Explanation:

$NH_{3}(g) + O_{2}(g) \: → NO_{2} + H_{2}O(g)$

__↑______↑

8.00 mol | 14.00 mol

________________

$NH_{3}(g) + O_{2}(g) \: → NO_{2} + H_{2}O(g)$

You can turn this into a system of variables which are solvable.

To do this, create variables for the coefficients of each compound in the reaction respectively.

$a(NH_{3}(g)) + b(O_{2}(g)) → \\c(NO_{2}) + d(H_{2}O(g))$

Because to be balanced, the count of atoms in each element of the compound correspond to the coefficient of the variable in that compound so that the count of the left (reactant) side is set equal to the right (product) side.

a corresponds to the coefficient of the first compound, b corresponds to the coefficient of the second compound, c corresponds to the coefficient of the third compound, and d corresponds to the coefficient of the fourth compound.

(Reactant = Product)

Reactant: 1a [N] Product: 1c.

Reactant: 3a [H] Product: 2d.

Reactant: 2b [O] Product: 2c + 1d.

Thus the system is:

1a = 1c

3a = 2d

2b = 2c + 1d.

Then just use the substitution methods to solve.

3 0

2 years ago

Give the formula

madreJ [45]

Hello!!! I would like to give you my answer!!!
<span>%error= (-890kJ-0.07kJ)/(-890kJ)x100 = 110.02%
I hope this helps!!! :-D</span>

8 0

3 years ago