Chemistry High School

How many moles of helium are needed to fill a balloon to a volume of 6.3 L at 28 °C and 320
mmHg?
Round answer to 0.01 decimals

Answers

Answer 1

Answer:

.11 mol

Explanation:

Convert mmHg to atms by dividing by 760. Then multiply 6.3 by the atms and divide by .08206*(273+28) to get mol

Answer 2
.11 mol is the answer

Related Questions

When this gas is burned what will happen to the surface of this type of star?

Answers

Use the link above for the answer

THIS IS FOR SCIENCE PLS HELP ME WRITE MY PROMPT How does the human population and human activity affect Earth?

Answers

both work together and the human activity is what population counts on and the activity is what effects the population

11) How many grams are in 2.3 moles of magnesium chloride, MgCl,?

Answers

Answer:

218.98 grams

Explanation:

Given that,

No. of moles, n = 2.3

The molar mass of magnesium chloride is 95.211 g/mol.

We need to find the mass of 2.3 moles of magnesium chloride.

We know that,

No. of moles = given mass/molar mass

Let m be the given mass. So,

[tex]m=n\times M\\\\=2.3\times 95.211 \\\\=218.98\ g[/tex]

So, the required mass is equal to 218.98 grams.

When 1 mol of Zn reacts with 0.8 mol of HCI, which of the following will be true?

Answers

Answer:

Zn is the excess reagent

Explanation:

a 5 g ice cube starts life at -1 C if 2182.5 j are added to it what will be the final temperature upon his demise ?

Answers

Answer:

Final Temp = 23.92°C

Explanation:

ΔH(total) = (m·c·ΔT)ice + (m·ΔH(f))melt'g + (m·c·ΔT)water

2182.5j = (5g)(2.092j/g·°C)(1°C) + (5g)(334.56j/g) + (5g)(4.184j/g·°C)(ΔT)

(2182.5 - 10.46 - 1672.8)j = 20.92j/°C·ΔT

ΔT = (2182.5 - 10.46 - 1672.8)j / 20.92j/°C = 23.92°C

Since the melting ice starts and ends at 0°C and is then warmed to 23.92°C then the temperature change is also the final temp of the water based upon given energy input values.

When(NH4)2SO4(aq) and Ba(NO3)2(aq) react

Answers

Answer:

1 (NH4)2SO4 + Ba(NO3)2 → NH4NO3 + BaSO4

2 (NH4)2SO4 + Ba(NO3)2 → Ba(SO4) + (NH4)(NO3)

Explanation:


A reaction in the laboratory yields 5.98 g KAI(SO2)2, How many moles of potassium aluminum
sulfate were produced?

Answers

Answer:

0.0308 mol

Explanation:

In order to convert from grams of any given substance to moles, we need to use its molar mass:

Molar mass of KAI(SO₂)₂ = MM of K + MM of Al + (MM of S + 2*MM of O)*2Molar mass of KAI(SO₂)₂ = 194 g/mol

Now we calculate the number of moles of KAI(SO₂)₂ contained in 5.98 g:

5.98 g ÷ 194 g/mol = 0.0308 mol

Which statement describes particles of an ideal gas, based on the kinetic molecular theory?

Answers

Answer:

There are 5 steps/rules of the ideal gases based on kinetic theory.

Explanation:

1. Particles in a gas are constant moving in random motion.

2. combined volume of the particles is negligible.

3. particles exert no forces on one another

4. any collisions between the particles are completely elastic

5. the average kinetic energy of particles is proportional to temperature in kelvins.

(I had help explaining steps from Sal Khan. I hope this helps! Have a great day!)

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