All categories

4 years ago

If a sample of gallium totals 1.22 mol, what is the mass of the sample?

Chemistry

2 answers:

Alexandra [31]4 years ago

6 0

Answer:

The answer to your question is the letter a. 85.06 g

Explanation:

Data

1.22 moles of Ga

Process

1.- Look for the Atomic mass of Ga in the periodic table

Atomic mass = 69.72 g

2.- Use proportions to calculate the moles of Ga

69.72 g ------------------- 1 mol

x ------------------- 1.22 moles

x = (1.22 x 69.72) / 1

x = 85.06/ 1

x = 85.06 g og Ga

Lunna [17]4 years ago

3 0

Answer:

The mass of this gallium sample is 85.06 grams ( option A is correct).

Explanation:

Step 1: Data given

Number of moles of galium = 1.22 moles

Atomic mass of galium = 69.723 g/mol

Step 2: Calculate mass of gallium

Mass of gallium = moles gallium * molar of gallium

Mass of gallium = 1.22 moles * 69.723 g/mol

Mass of gallium = 85.062 ≈ 85.06 grams

The mass of this gallium sample is 85.06 grams ( option A is correct).

You might be interested in

A year has 365 days, and a day has 24 hours. If an hour has 60 minutes and a minute has 60 seconds, how many seconds are there i

Cloud [144]

Answer:

31,536,000 seconds

Explanation:

off google

3 0

3 years ago

Read 2 more answers

A sample of gas occupies a volume of 61.5 mL . As it expands, it does 130.1 J of work on its surroundings at a constant pressure

Lesechka [4]

Answer:

the final volume of the gas is $V_2$ = 1311.5 mL

Explanation:

Given that:

a sample gas has an initial volume of 61.5 mL

The workdone = 130.1 J

Pressure = 783 torr

The objective is to determine the final volume of the gas.

Since the process does 130.1 J of work on its surroundings at a constant pressure of 783 Torr. Then, the pressure is external.

Converting the external pressure to atm ; we have

External Pressure $P_{ext}$ :

$P_{ext} = 783 \ torr \times \dfrac{1 \ atm}{760 \ torr}$

$P_{ext} = 1.03 \ atm$

The workdone W = $P_{ext}$ V

The change in volume ΔV= $\dfrac{W}{P_{ext}}$

ΔV = $\dfrac{130.1 \ J \times \dfrac{1 \ L \ atm}{ 101.325 \ J} }{1.03 \ atm }$

ΔV = $\dfrac{1.28398717 }{1.03 }$

ΔV = 1.25 L

ΔV = 1250 mL

Recall that the initial volume = 61.5 mL

The change in volume V is $\Delta V = V_2 -V_1$

$- V_2= - \Delta V -V_1$

multiply through by (-), we have:

$V_2= \Delta V+V_1$

$V_2$ = 1250 mL + 61.5 mL

$V_2$ = 1311.5 mL

∴ the final volume of the gas is $V_2$ = 1311.5 mL

5 0

3 years ago

The bulk of nuclear waste is in the form of ______

Alina [70]

Answer:

The bulk of nuclear waste is in the form of <u>solid ceramic pellets</u>.

Explanation:

Nuclear fuel loaded into commercial reactors is generally in the form of solid ceramic pellets that are stacked into metal tubes and bundled together in fuel assemblies. After the atoms in the pellet split to release their energy, the pellets in tubes emerge as nuclear waste.

Pls, choose me as brainliest!

7 0

3 years ago

Write balanced net ionic equations and the corresponding equilibrium equations for the stepwise dissociation of the triprotic ac

Elza [17]

Answer:

$H_3PO_4(aq)+H_2O(l)\rightleftharpoons H_3O^+(aq)+H_2PO_4^{-}(aq); \ Ka_1$

$H_2PO_4^{-}(aq)+H_2O(l)\rightleftharpoons H_3O^+(aq)+HPO_4^{-2}(aq); \ Ka_2$

$HPO_4^{-2}(aq)+H_2O(l)\rightleftharpoons H_3O^+(aq)+PO_4^{-3}(aq); \ Ka_3$

Explanation:

Hello!

In this case, since the phosphoric acid is a triprotic acid, we infer it has three stepwise ionization reactions in which one hydrogen ion is released at each step, considering they are undergone due to the presence of water, thus, we proceed as follows:

$H_3PO_4(aq)+H_2O(l)\rightleftharpoons H_3O^+(aq)+H_2PO_4^{-}(aq); \ Ka_1$

$H_2PO_4^{-}(aq)+H_2O(l)\rightleftharpoons H_3O^+(aq)+HPO_4^{-2}(aq); \ Ka_2$

$HPO_4^{-2}(aq)+H_2O(l)\rightleftharpoons H_3O^+(aq)+PO_4^{-3}(aq); \ Ka_3$

Moreover, notice each step has a different acid dissociation constant, which are quantified in the following order:

Ka1 > Ka2 > Ka3

Best regards!

3 0

3 years ago

How many molecules are indicated by writing 2 H2O

scoundrel [369]

There are 2 molecules indicated

8 0

3 years ago

Read 2 more answers