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2 years ago

Consider the reaction below.

1 answer:

6 0

This answer to this question is a rule that is applied to any reaction taken at dynamic equilibrium, with respect to 500 K. In other words, you can say that this reaction is of no use to us -

In a chemical equilibrium, it is known that the forward and reverse reactions occur at equal rates. At this point the concentrations of products and reactants remain constant, or in other words do not change

Solution = Option C

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The mass number of an atom can be calculated from the

11111nata11111 [884]

Mass number (A) =protons (p+) + neutrons(n°)

8 0

2 years ago

A sleeping 68 kg man has a metabolic power of 65 w . you may want to review ( pages 323 - 327) . part a how many calories does h

Kazeer [188]

Given:

Mass = 68 kg

Power = 65 W

To determine:

Calories burned during an 8.0 hr sleep

Explanation:

Energy is expressed as:

Energy = Power * Time

Now, the unit of power = Watt (W)

1 W = 1 J/s i.e. 65 W = 65 J/s

Time = 8 hrs = 8 * 3600 s = 28800 s

Energy = 65 J/s * 28800 s = 1872000 J

Convert Joules (J) to calories (cal)

1 cal = 4.184 J

The calculated energy = 187200 J * 1 cal/4.184 = 447418 cal

Ans: The man burns nearly 447.4 kcal during an 8 hr sleep

8 0

3 years ago

a cylinder with a movable piston contains 250 cm3 air at 10°C. if the pressure is kept constant, at what temperature would you e

soldi70 [24.7K]

Answer:

T₂ = 169.89 K

Explanation:

Given data:

Initial volume = 250 cm³

Initial temperature = 10°C (10+273.15 K = 283.15 K)

Final temperature = ?

Final volume = 150 cm³

Solution:

The given problem will be solve through the Charles Law.

According to this law, The volume of given amount of a gas is directly proportional to its temperature at constant number of moles and pressure.

Mathematical expression:

V₁/T₁ = V₂/T₂

V₁ = Initial volume

T₁ = Initial temperature

V₂ = Final volume

T₂ = Final temperature

Now we will put the values in formula.

V₁/T₁ = V₂/T₂

T₂ = T₁V₂/V₁

T₂ = 283.15 K × 150 cm³ / 250 cm³

T₂ = 42472.5 K. cm³ / 250 cm³

T₂ = 169.89 K

5 0

2 years ago

a quantity of zinc reacts with sulfuric acid and produces 0.10g of hydrogen. how many particles of zinc are required socratic.or

alekssr [168]

Answer:

grams of zinc required = 3.24 g

Particles of zinc required = $2.99\times 10^{22}$

Explanation:

Given that:-

Mass of hydrogen gas produced = 0.10 g

Calculation of the moles of $H_2$ as:-

Mass = 0.10 g

Molar mass of $H_2$ = 2.016 g/mol

The formula for the calculation of moles is shown below:

$moles = \frac{Mass\ taken}{Molar\ mass}$

Thus,

$Moles= \frac{0.10\ g}{2.016\ g/mol}$

$Moles= 0.0496\ mol$

According to the reaction shown below:-

$Zn+H_2SO_4\rightarrow ZnSO_4+H_2$

1 mole of hydrogen gas is produced when 1 mole of zinc reacts

So,

0.0496 mole of hydrogen gas is produced when 0.0496 mole of zinc reacts

Moles of Zinc required = 0.0496 moles

Molar mass of zinc = 65.38 g/mol

mass= Moles*Molar mass = $0.0496\ moles\times 65.38\ g/mol=3.24\ g$

Also, 1 mole of Zinc contains $6.023\times 10^{23}$ particles

0.0496 mole of Zinc contains $0.0496\times 6.023\times 10^{23}$ particles

Particles of zinc required = $2.99\times 10^{22}$

6 0

2 years ago

Can someone help me with this?

Rudik [331]

Yeah so you have to start of with converting your first two values into moles (forget the third one)

97.5 g NO * 1 mol/30.01 g NO = 3.25 moles NO

88.0 g O2 * 1 mol/16.00 g O2 = 5.5 moles O2

now we can find the limiting reactant by checking for the amount of product each reactant should give us by using molar ratios

3.25 mol NO * 2 mol NO2/2 mol NO = 3.25 mol NO2

5.5 mol O2 * 2 mol NO2/ 1 mol O2 = 11

so NO is the limiting reactant since it produces less product/gets used up quicker

3.25 mol NO * 2 mol NO2/2molNO = 3.25 mol NO2

so this is our theoretical yield and the question provides us with the actual yield (2.68 moles). since the actual yield is given in moles, we don't have to convert to grams. our percent yield formula goes like: actual yield/theoretical yield * 100

2.68 mol/3.25 mol * 100 = 82.46%

4 0

2 years ago