All categories

4 months ago

Enter the chemical equation 2H+(aq)+S2−(aq)→H2S(g). Express your answer as a chemical equation.

Chemistry

2 answers:

VMariaS [2.9K]4 months ago

6 0

Here is the chemical equation: 2H⁺(aq) + S²⁻(aq) → H₂S(g) $2H^+ (aq) + S^{2-}(aq) => H_2S(g)$

Additional explanation

Writing chemical equations is a key skill in chemistry, as they portray reactions between substances. The reactants appear on the left side, products on the right, with an arrow indicating the transformation.

The phases of substances are included inside parentheses as subscripts.

When ions are involved, superscripts denote their charges, with numbers placed before the charge (e.g., 2+, not +2).

The complete balanced chemical equation with phases for the given reaction is:

$2H^+ (aq) + S^{2-}(aq) => H_2S(g)$

Sulfur $S$ is a chemical element symbolized by S with atomic number 16; it is abundant, multivalent, and nonmetallic. Hydrogen sulfide $H_2S$ is a colorless gas that is highly toxic, corrosive, and flammable. Hydrogen $H$ is the most plentiful chemical element in the universe.

Learn more

About chemical equations: brainly.com/question/12271256
About Hydrogen sulfide: brainly.com/question/12592944
About Sulfur: brainly.com/question/4288925

Answer details

Grade: 9

Subject: Chemistry

Chapter: the chemical equation

Keywords: chemical equation, Introduction to Mastering Chemistry, Chemistry, equation, Hydrogen sulfide

Anarel [2.9K]4 months ago

4 0

Answer: The complete balanced chemical equation is,

$2H^+(aq)+S^{2-}(aq)\rightarrow H_2S(aq)$

Explanation:

A chemical equation represents the reactants on the left and the products on the right, separated by a right-pointing arrow indicating the reaction.

This representation includes the phases of the substances and uses subscripts and superscripts for numbers.

For the reaction given, the balanced chemical equation with phases is:

$2H^+(aq)+S^{2-}(aq)\rightarrow H_2S(aq)$

You might be interested in

An electrochemical cell is constructed with a zinc metal anode in contact with a 0.052 M solution of zinc nitrate and a silver c

Tems11 [2777]

Q is determined to be 12.38. The Nernst equation is expressed as Ecell = E°cell - (2.303RT/nF) log Q, where Q represents the reaction quotient. The reaction quotient Q is calculated by taking the product of the products' concentrations divided by the product of the reactants' concentrations. For an electrochemical cell, Q is the concentration ratio of the solution at the anode compared to that at the cathode. Consequently, Q = [anode]/[cathode], specifically Q = 0.052/0.0042, arriving at a value of Q = 12.38.

6 0

3 months ago

A chamber with a fixed volume is shown above. The temperature of the gas inside the chamber before heating is 25.2 C and it’s pr

KiRa [2933]

Answer:

Explanation:

Given data:

Initial temperature T₁ = 25.2°C = 298.2K

Initial pressure P₁ = 0.6atm

Final temperature = 72.4°C = 345.4K

What we need to find:

Final pressure = ?

To determine this, we apply a modified version of the combined gas law with constant volume. This simplifies our calculations to:

$\frac{P_{1} }{T_{1} } = \frac{P_{2} }{T_{2} }$

Here, P and T signify pressure and temperatures, 1 refers to initial and 2 to final temperatures.

Now we can substitute the known variables:

$\frac{0.6}{298.2} = \frac{P_{2} }{345.4}$

P₂ = 0.7atm

3 0

4 months ago

An industrial manufacturer wants to convert 175 kg of methane into HCN. Calculate the masses of ammonia and molecular oxygen req

Alekssandra [3086]

Context:

175 kilograms of methane (CH4) is to be converted into hydrogen cyanide (HCN)

The equation that balances this reaction is listed here:

2 CH4 + 2 NH3 + 3 O2 → 2 HCN + 6 H2O

To find the quantities of ammonia and oxygen needed, we will use 175 kg of CH4 as our reference.

Molar masses are as follows:
CH4 = 16 kg/kmol
NH3 = 17 kg/kmol
O2 = 32 kg/kmol

For ammonia: mass of NH3 = 175 kg CH4 / 16 kg/kmol * (2/2) * 17 kg/kmol
This results in 185.94 kg of NH3 required

For oxygen: mass of O2 = 175 kg CH4 / 16 kg/kmol * (3/2) * 32 kg/kmol
So the mass of O2 needed equals 525 kg

To derive the mass of oxygen: mass of O = 525 kg / 32 kg/kmol * (1/2) * 16 kg/kmol
This gives a mass of O equal to 131.25 kg O

4 0

3 months ago