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3 years ago

What is described in the following equation?

Chemistry

1 answer:

Alexus [3.1K]3 years ago

8 0

Answer:

A. Hydrogen gas combining with oxygen gas to form water.

Explanation:

H2 is the symbol for Hydrogen in gaseous state and O2 is the symbol for Oxygen in gaseous state. H2O is the chemical formula of Water. It is clearly indicated in the equation that Hydrogen and Oxygen combining to form Water.

The arrow to the water indicate that the water is the product and it is NOT the decomposition reaction.

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Zinc metal is added to a flask containing aqueous hydrochloric acid. The flask contains 0.400 mole of HCl. How much hydrogen gas

dusya [7]

Answer:

0.4 g of hydrogen gas would be produced.

1. 0.48 mole of HCl is needed to react completely with 15.5 g of zinc.

2. HCl is the limiting reactant.

3. 2.61 g of zinc is in excess

Explanation:

From the balanced equation of reaction:

$Zn(s)+ 2HCl(aq) --> H_2(g) + ZnCl_2(aq)$

1 mole of Zn requires 2 moles of HCl to produce 1 mole of hydrogen gas.

15.5 g of zinc = 15.5/65.3 = 0.24 moles of zinc.

0.24 moles Zn is supposed to require 0.24 x 2 moles HCl which is equivalent to 0.48 moles HCl.

But only 0.400 mole of HCl is present. Hence, HCl is the limiting reagent. For complete reaction with 15.5 g of Zinc, 0.48 mole HCl would be needed.

0.400 mole of HCl will require 0.2 mole of Zn for complete reaction. This thus means that 0.24 - 02 = 0.04 mole of Zn is in excess.

0.04 mole Zn = 0.04 x 65.3 = 2.61 g excess Zn.

Now, since HCl is the limiting reagent;

2 moles of HCl is required to produce 1 mole of H2 according to the equation.

0.400 mole HCl will therefore yield 0.400 x 1/2 = 0.2 mole H2

0.2 mole H2 = 2 x 0.2 = 0.4 g H2

Hence, 0.4 g of hydrogen gas would be produced.

6 0

3 years ago

A steel tank contains carbon dioxide at a pressure of 13.0 atm when the temperature is 34oC. What will be the internal gas press

morpeh [17]

Answer:

D. 15.8atm

Explanation:

Given parameters:

Initial pressure = 13atm

Initial temperature = 34°C = 34 + 273 = 307K

Final temperature = 100°C = 100 + 273 = 373K

Unknown:

Final pressure = ?

Solution:

To solve this problem, we apply a derivation of the combined gas law taking the volume as a constant.

The expression is shown mathematically below;

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

P and T pressure and temperature values

1 and 2 are initial and final states

Insert the parameters and solve for T₂;

$\frac{13}{307}$ = $\frac{P_{2} }{373}$

P₂ = 15.8atm

4 0

3 years ago

60.0 mL of 0.0100 M H3PO4 are required to neutralize 30.0 mL of a solution of KOH. What is the molarity of the potassium hydroxi

Vsevolod [243]

Answer:

h2o

Explanation:

3 0

3 years ago

The molar heat of vaporization of water is 40.7kJ/mol. How much heat must be absorbed to convert 50.0 grams of liquid water at 1

EleoNora [17]

During a phase change the temperature does not change since all of the heat is being absorbed in order to break the intermolecular forces. Due to that, the formula will not need to have T in it and is actually q=nΔH(v).
n=the number of moles (in this case 2.778mol of water since you divide 50g by 18g/mol).
ΔH(v)=the molar heat of vaporization (in this case 40.7kJ/mol).
q=the heat that must be absorbed
q=2.778mol×40.7kJ/mol
q=113.1kJ
Therefore the water needs to absorb 1.13×10²kJ.

I hope this helps. Let me know if anything is unclear.

4 0

3 years ago

Please help thank you (15 points)

dsp73

Answer:

Explanation:

The arrows represent the Earth spinning on its own axis in this picture.

4 0

3 years ago