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2 years ago

An object accelerates 12.0 m/s2 when a force of 6.0 newtons is applied to it. What is the mass of the object?

Chemistry

1 answer:

dedylja [7]2 years ago

5 0

Answer:

The mass of object is 0.5 Kg.

Explanation:

Given data:

Acceleration of object = 12.0 m/s²

Force on object = 6.0 N

Mass of object = ?

Solution:

Formula:

F = m×a

F = force

m = mass

a = acceleration

Now we will put the values in formula.

6.0 N = m × 12.0 m/s²

m = 6.0 N / 12.0 m/s²

( N = kg.m/s²)

m = 0.5 kg

The mass of object is 0.5 Kg.

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A ground state hydrogen atom absorbs a photon of light having a wavelength of 93.7 nm.93.7 nm. What is the final state of the hy

sammy [17]

Answer:

Explanation:

Given that the formula is;

1/λ= R(1/nf^2 - 1/ni^2)

λ = 93.7 nm or 93.7 * 10^-9 m

R= 1.097 * 10^7 m-1

nf = ?

ni = 1

From;

ΔE = hc/λ

ΔE = 6.63 * 10^-34 * 3* 10^8/93.7 * 10^-9

ΔE = 21 * 10^-19 J

ΔE = -2.18 * 10^-18 J (1/nf^2 - 1/ni^2)

21 * 10^-19 J = -2.18 * 10^-18 J (1/nf^2 - 1/ni^2)

21 * 10^-19/-2.18 * 10^-18 = (1/nf^2 - 1/1^2)

-0.963 = (1/nf^2 - 1)

-0.963 + 1 = 1/nf^2

0.037 = 1/nf^2

nf^2 = (0.037)^-1

nf^2 = 27

nf = 5

7 0

2 years ago

1. Which liquid sample is a pure substance?

IRISSAK [1]

The whole Activity , poem and paragraph is missing in the question.

Answer:

(1) Liquid A

(2) Solid A

Explanation:

Using this part of the given poem

Substances and mixtures behave differently,

During boiling and melting most especially

Boiling point of substance is fixed while mixture is not

Substance melts completely but mixture does not

The boiling point of the Pure substance remain fixed after reaching its boiling point this is shown by Liquid A

Solid A is melting completely so Solid A is a pure substance.

6 0

2 years ago

What is the mass of 2.5 moles of hydrogen fluoride gas HF

Nady [450]

Answer:

You will get 5.0 g of hydrogen.

Explanation:

As with any stoichiometry problem, we start with the balanced equation.

2HF

→

SnF

Moles of H

2.5

mol Sn

1 mol H

mol Sn

2.5 mol H

Mass of H

2.5

mol H

2.016 g H

mol H

5.0 g H

7 0

2 years ago

A hypothetical substance has a melting point of −10°C and a boiling point of 155°C. If this substance is heated from 2°C to the

igor_vitrenko [27]

Answer:

The specific heat capacity of liquid and the het of vaporization is used.

Explanation:

Step 1: Data given

A substance at temperature 2°C.

The substance has a melting point of −10°C and a boiling point of 155°C.

The initial temperature is 2°C which is between the melting point (-10°C) and the boiling point (155°C). At 2°C, the substance is liquid.

At 155°C, the substance changes from liquid to gas.

To calculate the heat gained for the change of 2°C liquid to 155°C liquid, specific heat capacity of the liquid (C) is needed.

To calculate the heat gained for the change of liquid to 155°C gas, heat of vaporization (D) is needed.

The specific heat of the solid is not used because the substance is changed from liquid to gas. it doesn't come in the state of solid.

Heat of fusion is not used, because it's used when there is a change from its state from a solid to a liquid,

The specific heat capacity of the gas is not used, because the substance only formes gas after reaching 155 °C

5 0

2 years ago

SnO2 is reduced by carbon according to this reaction: SnO2 + C ???? Sn + CO2. How many liters of CO2 are produced if 300.0 grams

andrew-mc [135]

Explanation:

The given reaction is as follows.

$SnO_{2} + C \rightarrow Sn + O_{2}$

a). Molar mass of $SnO_{2}$ is [(mass of Sn) + (2 × mass of O)].

Therefore, molar mass of $SnO_{2}$ = (118.7 + 2 × 16) g/mol = 150.7 g/mol

Since, it is known that number of moles equal mass divided by molar mass. So, moles of Sn will be calculated as follows.

No. of moles = $\frac{mass}{molar mass of SnO_{2}}$

= $\frac{300 g}{150.7 g/mol}$

= 2.53 mol

As it is given that 1 mole of $SnO_{2}$ produces 1 moles of Sn and 1 moles of $CO_{2}$ . Hence, 2.53 moles of $SnO_{2}$ will also produce 2.53 moles of Sn and 2.53 moles of $CO_{2}$ .

Volume of 1 mole of $CO_{2}$ at STP is 22.4 L. Therefore, volume of 2.53 moles of $CO_{2}$ will be calculated as follows.

2.53 × 22.5 L = 56.67 L

Hence, 56.67 L of $CO_{2}$ are produced if 300.0 grams of tin are produced at STP.

b). Mass of tin is given as 1800.0 g. So, number of moles will be calculated as follows.

No. of moles = $\frac{mass}{molar mass of tin}$

= $\frac{1800.0 g}{118.7 g/mol}$

= 15.2 moles

As 15.2 moles of $SnO_{2}$ produces 15.2 moles of Sn. Therefore, weight of $SnO_{2}$ will be calculated as follows.

Mass = no. of moles × molar mass of $SnO_{2}$

= 15.2 moles × 150.7 g/mol

= 2290.64 g

Hence, 2290.64 grams of $SnO_{2}$ are required to produce 1800.0 grams of tin.

c). Mass of carbon given is 100.0 grams.

No. of moles = $\frac{mass}{molar mass of carbon}$

= $\frac{100 g}{12 g/mol}$

= 8.33 moles

As, 1 mole of carbon is produced by 1 mole of tin. So, 8.33 mole of carbon will be produced by 8.33 moles of tin.

Therefore, calculate mass of tin produced as follows.

Mass = no. of moles × molar mass of Sn

= 8.33 moles × 118.7 g/mol

= 988.8 g

Hence, 988.8 grams of tin will be produced per 100 grams of carbon used.

8 0

2 years ago