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3 years ago

Can you help me please

Chemistry

1 answer:

9966 [12]3 years ago

8 0

Answer:

I think its, balanced chemical equations

Explanation:

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A 0.708 g sample of a metal, M, reacts completely with sulfuric acid according to the reaction M ( s ) + H 2 SO 4 ( aq ) ⟶ MSO 4

ollegr [7]

Answer:

The metal has a molar mass of 65.37 g/mol

Explanation:

Step 1: Data given

Mass of the metal = 0.708 grams

Volume of hydrogen = 275 mL = 0.275 L

Atmospheric pressure = 1.0079 bar = 0.9947 atm

Temperature = 25°C

Vapor pressure of water at 25 °C = 0.03167 bar = 0.03126 atm

Step 2: The balanced equation

M(s) + H2SO4(aq) ⟶ MSO4 (aq) + H2(g)

Step 3: Calculate pH2

Atmospheric pressure = vapor pressure of water + pressure of H2

0.9947 atm = 0.03126 atm + pressure of H2

Pressure of H2 = 0.9947 - 0.03126

Pressure of H2 = 0.96344 atm

Step 4: Calculate moles of H2

p*V=n*R*T

⇒ with p = The pressure of H2 = 0.96344 atm

⇒ with V = the volume of H2 = 0.275 L

⇒ with n = the number of moles H2 = TO BE DETERMINED

⇒ with R = the gas constant = 0.08206 L*atm/K*mol

⇒ with T = the temperature = 25°C = 298 Kelvin

n = (p*V)/(R*T)

n = (0.96344 * 0.275)/(0.08206*298)

n = 0.01083 moles

Step 5: Calculate moles of M

For 1 mole of H2 produced, we need 1 mole M

For 0.0108 moles of H2 we need 0.01083 moles of M

Step 6: Calculate molar mass of M

Molar mass M = Mass M / moles M

Molar mass M = 0.708 grams / 0.01083 moles

Molar mass M = 65.37 g/mol

The metal has a molar mass of 65.37 g/mol

5 0

4 years ago

What does the energy turn into when a lamp goes from unplugged to plugged

Zielflug [23.3K]

Kinetic Energy into Potential Energy

5 0

3 years ago

Read 2 more answers

Select all the correct answers.

OlgaM077 [116]

Answer:

It's The amount of matter within the system remains the same and The cycle has a well-defined starting and stopping point.

Explanation:

7 0

3 years ago

The pH of a solution is 8.83±0.048.83±0.04 . What is the concentration of H+H+ in the solution and its absolute uncertainty?

slava [35]

Answer:

The concentration of $H^{+}$ is 1.48 × $10^{-9}$ M

The absolute uncertainty of $[{H^{+}]$ is ±0.12 × $10^{-9}$ M

The concentration of $H^{+}$ is written as 1.48(±0.12) × $10^{-9}$ M

Explanation:

The pH of a solution is given by the formula below

pH = $-log_{10}[{H^{+}]$

∴ $[H^{+}] = 10^{-pH}$

where $[{H^{+}]$ is the $H^{+}$ concentration

From the question,

pH = 8.83±0.04

That is,

pH =8.83 and the uncertainty is ±0.04

First, we will determine $[{H^{+}]$ from

$[H^{+}] = 10^{-pH}$

$[{H^{+}] = 10^{-8.83}$

$[{H^{+}] = 1.4791$ × $10^{-9}$ M

$[{H^{+}] = 1.48$ × $10^{-9}$ M

The concentration of $H^{+}$ is 1.48 × $10^{-9}$ M

The uncertainty of $[{H^{+}]$ ( $U_{[H^{+}] }$ ) from the equation $[H^{+}] = 10^{-pH}$ is

$U_{[H^{+}] } = 2.303 \\$ × ${[H^{+}] }$ × $U_{pH }$

Where $U_{[H^{+}] }$ is the uncertainty of $[{H^{+}]$

$U_{pH }$ is the uncertainty of the pH

Hence,

$U_{[H^{+}] }$ = 2.303 × 1.4791 × $10^{-9}$ × 0.04

$U_{[H^{+}] }$ = 1.36 × $10^{-10}$ M

$U_{[H^{+}] }$ = 0.12 × $10^{-9}$ M

Hence, the absolute uncertainty of $[{H^{+}]$ is ±0.12 × $10^{-9}$ M

6 0

4 years ago

Question

rosijanka [135]

Answer:

there you go

Explanation:

6 0

3 years ago

Can you help me please ​

Can you help me please