All categories

3 years ago

In this activity, you will be observing a reaction where copper and silver nitrate react to form copper (II) nitrate and silver.

Chemistry

1 answer:

aalyn [17]3 years ago

4 0

Answer:

Copper(II) nitrate and silver

Explanation:

2AgNO₃(aq ) + Cu (s) --> Cu(NO₃)₂(aq ) + 2Ag(s)

This can be called a redox reaction because silver nitrate is reduced and copper is oxidized. This can also be called a single replacement reaction because copper replaces silver in the substance silver nitrate.

You might be interested in

In the dehydration of hydrated salt the sample was slightle moist because of high humidity briefly explain how the moisture affe

jenyasd209 [6]

Answer:

identify and name the landforms in the following diagrams

8 0

3 years ago

Which of the following is true about chemical reactions. A. they are accompanied by changes in energy. B. they form new substanc

Ilia_Sergeevich [38]

The correct answer should be option C. hope this helps

7 0

4 years ago

What is (3 X 10^3) +(2.5 X 10^6)? *

DaniilM [7]

Answer:

Scientific Notation: 2.503 × 10⁶

Standard Form: 2,503,000

5 0

3 years ago

Read 2 more answers

List the official SI units

Juli2301 [7.4K]

Answer:

The seven SI base units, which are comprised of:

Length - meter (m)

Time - second (s)

Amount of substance - mole (mole)

Electric current - ampere (A)

Temperature - kelvin (K)

Luminous intensity - candela (cd)

Mass - kilogram (kg)

Explanation:

7 0

4 years ago

Read 2 more answers

A certain substance X has a normal freezing point of -10.1 degree C and a molal freezing point depression constant Kf = 5.32 °C.

Citrus2011 [14]

Answer : The freezing point of a solution is $-15.4^oC$

Explanation : Given,

Molal-freezing-point-depression constant $(K_f)$ = $5.32^oC/m$

Mass of urea (solute) = 29.82 g

Mass of solvent = 500 g = 0.500 kg

Molar mass of urea = 60.06 g/mole

Formula used :

$\Delta T_f=i\times K_f\times m\\\\T^o-T_s=i\times K_f\times\frac{\text{Mass of urea}}{\text{Molar mass of urea}\times \text{Mass of solvent in Kg}}$

where,

$\Delta T_f$ = change in freezing point

$\Delta T_s$ = freezing point of solution = ?

$\Delta T^o$ = freezing point of solvent = $-10.1^oC$

i = Van't Hoff factor = 1 (for urea non-electrolyte)

$K_f$ = freezing point constant = $5.32^oC/m$

m = molality

Now put all the given values in this formula, we get

$-10.1^oC-T_s=1\times (5.32^oC/m)\times \frac{29.82g}{60.06g/mol\times 0.500kg}$

$T_s=-15.4^oC$

Therefore, the freezing point of a solution is $-15.4^oC$

5 0

3 years ago