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2 years ago

What mass of water can be made from 24 grams of oxygen and 16 g of hydrogen?

Chemistry

1 answer:

tangare [24]2 years ago

3 0

Answer:

27.025 g of H₂O

Explanation:

The Balance chemical equation is

2 H₂ + O₂ = 2 H₂O

Step 1: Calculate Limiting Reagent

Moles of H₂

Mole = 16 g / 2.02 g/mol = 7.937 mol

Moles of O₂

Mole = 24 g / 32.00 g/mol = 0.750 mol

Mole ratio of H₂ : O₂ is 2 : 1. Hence, 7.937 mol of H₂ will need 3.9685 mol of O₂. This means O₂ is limiting reagent.

Step 2: Calculate Moles of H₂O

0.750 mol of O₂ will produce 1.50 mol of H₂O because the mole ratio of O₂ : H₂O is 1 : 2.

Step 3: Calculate mass of H₂O

Mass = 1.50 mol × 18.02 g/mol = 27.025 g of H₂O

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3 years ago

A blood sample of 4.01 milliliters is collected from a patient to be analyzed for a platelet count. Human blood should have arou

Harlamova29_29 [7]

Given :

Human blood should have around 1.04 kg/L platelets.

A blood sample of 4.01 milliliters is collected from a patient to be analyzed for a platelet count.

To Find :

The expected mass in grams of platelets in the blood sample.

Solution :

1 L of human blood contains 1.04 kg of platelets.

So, amount of platelets is 1 ml blood is :

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3 years ago

If 4.50 l of water vapor at 50.2 °c and 0.121 atm reacts with excess iron, how many grams of iron(iii) oxide will be produced?

Flura [38]

When the balanced equation for this reaction is:
2Fe + 3H2O → Fe2O3 + 3H2

and according to the vapour pressure formula:
PV= nRT
when we have P is the vapor pressure of H2O= 0.121 atm
and V is the volume of H2O = 4.5 L
and T in Kelvin = 52.5 +273 = 325.5 K
R= 0.08205 atm-L/g mol-K
So we can get n H2O
So, by substitution:
n H2O = PV/RT
= (0.121*4.5)/(0.08205 * 325.5) = 0.02038 gmol
n Fe2O3 = 0.02038 * (1Fe2O3/ 3H2O) = 0.00679 gmol
Note: we get (1FeO3/3H2O) ratio from the balanced equation.
we can get the Mass of Fe2O3 from this formula:
Mass = number of moles * molecular weight
when we have a molecular weight of Fe2O3 = 159.7
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6 0

3 years ago

Read 2 more answers

Oxygen gas, generated by the reaction 2KClO3(s)---2KCl(s)+3O2(g), is collected over water at 27•C in 3.72L vassel at a total pre

Julli [10]

Answer:

moles = 0.093 moles

Explanation:

In this case, we know that this reaction is taking plave in a vessel that has a 730 torr of total pressure.

The total pressure is a value obtained by:

Pt = Pwater + PO2

We need to know the pressure of O2, because then, with stoichiometry, we can calculate the moles of KClO3

The pressure of oxygen is:

PO2 = 730 - 26 = 704 Torr

Now, this pressure is in Torr, and we need to convert it to Atm, so:

704 Torr / 760 Torr = 0.9263 atm

Now, let's use the ideal gas equation:

PV = nRT

With this expression, we will calculate the moles of O2, and then, the moles of KClO3:

n = PV/RT

R = 0.082 L atm /K mol

P = 0.9263 atm

V = 3.72 L

T = 27 + 273 = 300 K

Replacing the data:

n = 0.9263 * 3.72 / 300 * 0.082

n = 0.14 moles

Finally, by stoichiometry, we know that 2 moles of KClO3 produces 3 moles of O2, so:

moles of KClO3 = 0.14 * 2/3 = 0.093 moles of KClO3

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3 years ago

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Eva8 [605]

Answer:

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