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2 years ago

For the balanced equation shown below, how many moles of CO2 will react with 0.708 moles of H2O.

Chemistry

1 answer:

fgiga [73]2 years ago

7 0

Answer:

0.5 moles of CO2 will react with 0.708 moles of H2O.

Explanation:

$\sf balanced \ equation = 3CO2 + 4H2O \rightarrow C3H8 + 5O2$

0.708 moles of H2O

using molar ratio:

4H2O : 3CO2

4 : 3

so H2O moles:

$\sf\dfrac{0.708}{4} *3$

$\sf 0.531$ moles of CO2

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A solution is prepared by dissolving 0.7234 g oxalic acid (H2C2O4) in enough water to make 100.0 mL of solution. A 10.00-mL aliq

marishachu [46]

Answer: The final molarity of the diluted oxalic acid solution is 0.0032 M

Explanation:

Molarity: It is defined as the number of moles of solute present per liter of the solution.

Formula used :

$Molarity=\frac{n\times 1000}{V_s}$

where,

n= moles of solute

Moles= $\frac{\text{Given mass}}{\text{Molar mass}}=\frac{0.7234g}{90g/mol}=0.008moles$

$V_s$ = volume of solution in ml

$Molarity=\frac{0.008\times 1000}{100.0}=0.08$

To calculate the final molarity of the diluted oxalic acid solution

$M_1V_1=M_2V_2$

where,

$M_1\text{ and }V_1$ are the molarity and volume of concentrated oxalic acid solution.

$M_2\text{ and }V_2$ are the molarity and volume of diluted oxalic acid solution.

We are given:

$M_1=0.08\\V_1=10.00mL\\M_2=?\\V_2=250.0mL$

Putting values in above equation, we get:

$0.08\times 10.00=M_2\times 250.0\\\\M_2=0.0032M$

Thus the final molarity of the diluted oxalic acid solution is 0.0032 M

8 0

3 years ago

What is the mass of 22.4 L of H2O at STP?

Andrew [12]

Answer is: A. 18.02 g/mol.

At standard temperature and pressure 1 mol of gas occupied 22.4 liters:
V(H₂O) = 22.4 L; volume of water.
Vm = 22.4 L/mol; molar volume at STP.
n(H₂O) = V ÷ Vm.
n(H₂O) = 22.4 L ÷ 22.4 L/mol.
n(H₂O) = 1 mol; amount of substance (water).
M(H₂O) = Ar(O) + 2Ar(H) · g/mol.
M(H₂O) = 16 + 2 ·1.01 · g/mol.
M(H₂O) = 18.02 g/mol; molar mass of water.

3 0

3 years ago

Identify the limiting reactant in the reaction of nitrogen and hydrogen to form NH3 if 5.23 g of N2 and 5.52 g of H2 are combine

Marrrta [24]

Answer:

1) The limiting reactant is N₂ because it is present with the lower no. of moles than H₂.

2) The amount (in grams) of excess reactant H₂ = 4.39 g.

Explanation:

Firstly, we should write the balanced equation of the reaction:

N₂ + 3H₂ → 2NH₃.

1) To determine the limiting reactant of the reaction:

From the stichiometry of the balanced equation, 1.0 mole of N₂ reacts with 3.0 moles of H₂ to produce 2.0 moles of NH₃.

This means that N₂ reacts with H₂ with a ratio of (1:3).

We need to calculate the no. of moles (n) of N₂ (5.23 g) and H₂ (5.52 g) using the relation: n = mass / molar mass.

The no. of moles of N₂ in (5.23 g) = mass / molar mass = (5.23 g) / (28.00 g/mol) = 0.1868 mol.

The no. of moles of H₂ (5.52 g) = mass / molar mass = (5.52 g) / (2.015 g/mol) = 2.74 mol.

From the stichiometry, N₂ reacts with H₂ with a ratio of (1:3).

The ratio of the reactants of N₂ (5.23 g, 0.1868 mol) to H₂ (5.52 g, 2.74 mol) is (1:14.67).

∴ The limiting reactant is N₂ because it is present with the lower no. of moles than H₂.

0.1868 mol of N₂ react completely with 0.5604 mol of H₂ and the remaining of H₂ is in excess.

2) To determine the amount (in grams) of excess reactant of the reaction:

As showed in the part 1, The limiting reactant is N₂ because it is present with the lower no. of moles than H₂.

Also, 0.1868 mol of N₂ react completely with 0.5604 mol of H₂ and the remaining of H₂ is in excess.

The no. of moles are in excess of H₂ = 2.74 mol - 0.5604 mol (reacted with N₂) = 2.1796 mol.

∴ The amount (in grams) of excess reactant H₂ = n (excess moles) x molar mass = (2.1796 mol)((2.015 g/mol) = 4.39 g.

4 0

2 years ago

Which reaction will most likely take place based on the activity series? Li > K Ba CaNa > Mn > Zn > Cr> Fe> Cd

allsm [11]

Answer:

Among the given reactions,

a. Ag+FeCl 3

b, Zn + CaO

C. Ba+Na 2 CO 3

d . Cr+KNO3

which reaction is likely to take place based on the reactivity series?

Explanation:

The metal reactivity series is:

Li > K> Ba >Ca>Na > Mn > Zn > Cr> Fe> Cd Ni > H > Sb > Cu > Ag > Pd > Hg > Pt

The highly reactive metal will displace the less reactive metal from its compound during a displacement reaction.

a. Ag+FeCl 3

Ag is less reactive than Fe, so Ag cannot displace Fe from its compound.

This reaction also does not occur.

b, Zn + CaO

Zn is less reactive than Ca, so it cannot displace Ca from its compound.

This reaction does not occur.

C. Ba+Na 2 CO 3

Ba is more reactive than Na, so Ba displaces Na from its compound.

This reaction is possible.

d . Cr+KNO3

Cr is less reactive than K, so it cannot displace K from its compound.

Hence, This reaction is not possible.

Answer:

option c) Ba+Na 2 CO 3 -> BaCO3 +2Na

5 0

3 years ago

Where is almost all the mass of an atom

VashaNatasha [74]

The nucleus!! This is made up of protons and neutrons that each weigh about 1 amu.

Electrons are not found in the nucleus and weigh almost nothing so chemistry in school doesn’t bother with them :)

8 0

3 years ago