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eduard
2 years ago
12

The _________________ are either elements or compounds which are present prior to a chemical reaction.

Chemistry
2 answers:
Savatey [412]2 years ago
4 0
The missing word would be reactintes
mr Goodwill [35]2 years ago
3 0
Reactants would be the missing word in the sentence because they make up the products in a chemical reaction
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With the aid of a balanced chemical equation explain Chemical Reactions and the Types Of Chemical Reaction
e-lub [12.9K]

Answer:

Answers

1.)reactants: nitrogen and hydrogen; product: ammonia.

2.)reactants: magnesium hydroxide and nitric acid; products: magnesium nitrate and water.

3.)N 2 + 3H 2 → 2NH 3

4.)Mg(OH) 2 + 2HNO 3 → Mg(NO 3) 2 + 2H 2O.

5.)2NaClO 3 → 2NaCl + 3O 2

6.)4Al + 3O 2 → 2Al 2O 3

7.)N 2(g) + 3H 2(g) → 2NH 3(g)

Explanation:

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6 0
3 years ago
You have 16.7 grams of hydrogen and 15.4 grams of oxygen in a synthesis rxn. Which is the limiting reagent?
sleet_krkn [62]

Answer:

oxygen is limiting reactant

Explanation:

Given data:

Mass of hydrogen = 16.7 g

Mass of oxygen = 15.4 g

Limiting reactant = ?

Solution:

Chemical equation:

2H₂ + O₂   →   2H₂O

Number of moles of hydrogen:

Number of moles = mass/ molar mass

Number of moles = 16.7 g/ 2 g/mol

Number of moles = 8.35 mol

Number of moles of oxygen:

Number of moles = mass/ molar mass

Number of moles = 15.4 g/ 32 g/mol

Number of moles = 0.48 mol

Now we will compare the moles of both reactant with product,

                 

                             H₂           :          H₂O

                              2            :            2

                             8.35        :            8.35

                             O₂           :          H₂O

                               1            :            2

                             0.48        :        2×0.48 = 0.96 mol

The number of moles of water produced by oxygen are less so it will limiting reactant.

3 0
3 years ago
HELP ME WITH ONE OR BOTH OF THESE QUEATIONS PLEASEEEE
marta [7]

Answer:

2. 181.25 K.

3. 0.04 atm.

Explanation:

2. Determination of the temperature.

Number of mole (n) = 2.1 moles

Pressure (P) = 1.25 atm

Volume (V) = 25 L

Gas constant (R) = 0.0821 atm.L/Kmol

Temperature (T) =?

The temperature can be obtained by using the ideal gas equation as illustrated below:

PV = nRT

1.25 × 25 = 2.1 × 0.0821 × T

31.25 = 0.17241 × T

Divide both side by 0.17241

T = 31.25 / 0.17241

T = 181.25 K

Thus, the temperature is 181.25 K.

3. Determination of the pressure.

Number of mole (n) = 10 moles

Volume (V) = 5000 L

Temperature (T) = –10 °C = –10 °C + 273 = 263 K

Gas constant (R) = 0.0821 atm.L/Kmol

Pressure (P) =?

The pressure can be obtained by using the ideal gas equation as illustrated below:

PV = nRT

P × 5000 = 10 × 0.0821 × 263

P × 5000 = 215.923

Divide both side by 5000

P = 215.923 / 5000

P = 0.04 atm

Thus, the pressure is 0.04 atm

6 0
3 years ago
6. How many moles of water would require 92.048 kJ of heat to raise its temperature from 34.0 °C to 100.0 °C? (3 marks)​
scoray [572]

Taking into account the definition of calorimetry, 0.0185 moles of water are required.

<h3>Calorimetry</h3>

Calorimetry is the measurement and calculation of the amounts of heat exchanged by a body or a system.

Sensible heat is defined as the amount of heat that a body absorbs or releases without any changes in its physical state (phase change).

So, the equation that allows to calculate heat exchanges is:

Q = c× m× ΔT

where Q is the heat exchanged by a body of mass m, made up of a specific heat substance c and where ΔT is the temperature variation.

<h3>Mass of water required</h3>

In this case, you know:

  • Heat= 92.048 kJ
  • Mass of water = ?
  • Initial temperature of water= 34 ºC
  • Final temperature of water= 100 ºC
  • Specific heat of water = 4.186 \frac{J}{gC}

Replacing in the expression to calculate heat exchanges:

92.048 kJ = 4.186 \frac{J}{gC}× m× (100 °C -34 °C)

92.048 kJ = 4.186 \frac{J}{gC}× m× 66 °C

m= 92.048 kJ ÷ (4.186 \frac{J}{gC}× 66 °C)

<u><em>m= 0.333 grams</em></u>

<h3>Moles of water required</h3>

Being the molar mass of water 18 \frac{g}{mole}, that is, the amount of mass that a substance contains in one mole, the moles of water required can be calculated as:

amount of moles=0.333 gramsx\frac{1 mole}{18 grams}

<u><em>amount of moles= 0.0185 moles</em></u>

Finally, 0.0185 moles of water are required.

Learn more about calorimetry:

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8 0
2 years ago
What is the answer ?
Fantom [35]
The answer is C Does it propaget
4 0
3 years ago
Read 2 more answers
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