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3 years ago

An excess of mg(s) is added to 100.ml of 0.400 m hcl. at 0c and 1 atm pressure, what volume of h 2 (g) can be obtained?

1 answer:

5 0

The balanced equation for the reaction between Mg and HCl is as follows
Mg + 2HCl --> MgCl₂ + H₂
stoichiometry of HCl to H₂ is 2:1

number of HCl moles reacted - 0.400 mol/L x 0.100 L = 0.04 mol of HCl
since Mg is in excess HCl is the limiting reactant
number of H₂ moles formed - 0.04/2 = 0.02 mol of H₂

we can use ideal gas law equation to find the volume of H₂
PV = nRT
where
P - pressure - 1 atm x 101 325 Pa/atm = 101 325 Pa
V - volume
n - number of moles - 0.02 mol
R - universal gas constant - 8.314 Jmol⁻¹K⁻¹
T - temperature in Kelvin - 0 °C + 273 = 273 K
substituting these values in the equation

101 325 Pa x V = 0.02 mol x 8.314 Jmol⁻¹K⁻¹ x 273 K
V = 448 x 10⁻⁶ m³
V = 448 mL
therefore answer is
c. 448 mL

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Montano1993 [528]

Answer:

Yes, the investigations will reach similar conclusions about the reactivity of H2 and Cl2

Explanation:

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2. The law of multiple proportions is an extension of the law of definite composition, which states that compounds will consist of defined ratios of elements.

3. A reaction with more reactants will need more care because more products are produced, which can be toxic

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3 years ago

Calculate the volume of a 2.0 molar aqueous solution made from 14 miles of K2S

Vilka [71]

Answer:

volume is 7.0 liters

Explanation:

We are given;

Molarity of the aqueous solution as 2.0 M
Moles of the solute, K₂S as 14 moles

We are required to determine the volume of the solution;

We need to know that;

Molarity = Moles ÷ volume

Therefore;

Volume = Moles ÷ Molarity

Thus;

Volume of the solution = 14 moles ÷ 2.0 M

= 7.0 L

Hence, the volume of the molar solution is 7.0 L

5 0

3 years ago

Complete and balance the molecular equation, including the phases, for the reaction of aqueous potassium sulfate, k2so4, and aqu

Tju [1.3M]

The reaction between K₂SO₄(aq) and SrI₂(aq) produces KI(aq) and SrSO₄(s) as products.

The reaction is
K₂SO₄(aq) + SrI₂(aq) → KI(aq)+ SrSO₄(s)

To balance the equation both side of the reaction should have same number of atoms in each element.

Right hand side of the reaction has 1 K, 1 I, 1 Sr, 1 S and 4 O atoms while 2 K, 2 I, 1 Sr,1 S and 4 O present in left hand side of the reaction.
Hence, number of I atoms and number of K atoms are not balanced.
To balance the K atoms we should add 2 before KI. Then I atoms will be 2 at the right hand side.

Hence, the balanced reaction equation is
K₂SO₄(aq) + SrI₂(aq) → 2KI(aq)+ SrSO₄(s)

3 0

3 years ago

Read 2 more answers

When comparing the two chair conformations for a monosubstituted cyclohexane ring, which type of substituent shows the greatest

Aleksandr [31]

Answer:

See the explanation

Explanation:

In this case, we have to keep in mind that in the monosubstituted product we only have to replace 1 hydrogen with another group. In this case, we are going to use the methyl group $CH_3$ .

In the axial position, we have a more steric hindrance because we have two hydrogens near to the $CH_3$ group. If we have more steric hindrance the molecule would be more unstable. In the equatorial positions, we don't any interactions because the $CH_3$ group is pointing out. If we don't have any steric hindrance the molecule will be more stable, that's why the molecule will the equatorial position.

See figure 1

I hope it helps!

6 0

3 years ago

Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction:P4(g) + 10 Cl2(g) → 4PCl5(s) ΔH°

miskamm [114]

Answer: The $\Delta H^o_{rxn}$ for the reaction is -1835 kJ.

Explanation:

Hess’s law of constant heat summation states that the amount of heat absorbed or evolved in a given chemical equation remains the same whether the process occurs in one step or several steps.

According to this law, the chemical equation is treated as ordinary algebraic expressions and can be added or subtracted to yield the required equation. This means that the enthalpy change of the overall reaction is equal to the sum of the enthalpy changes of the intermediate reactions.

The given chemical reaction follows:

$P_4(g)+10Cl_2(g)\rightarrow 4PCl_5(s)$ $\Delta H^o_{rxn}=?$