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3 years ago

13

Zinc metal reacts with copper sulfate through the following

1 answer:

morpeh [17]3 years ago

5 0

Answer:

26.9

Explanation:

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Copper metal (Cu) reacts with silver nitrate (AgNO3) in aqueous solution to form Ag and Cu(NO3)2. An excess of AgNO3 is present.

leonid [27]

Stoichiometry time! Remember to look at the equation for your molar ratios in other problems.

31.75 g Cu | 1 mol Cu | 2 mol Ag | 107.9 g Ag         6851.65
⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻   →   ⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻⁻ = 107.9 g Ag
       ∅        | 63.5 g Cu | 1 mol Cu | 1 mol Ag              63.5

There's also a shorter way to do this: Notice the molar ratio from Cu to Ag, which is 1:2. When you plug in 31.75 into your molar mass for Cu, it equals 1/2 mol. That also means that you have 1 mol Ag because of the ratio, qhich you can then plug into your molar mass, getting 107.9 as well.

3 0

3 years ago

Read 2 more answers

10. When a sunlike star’s hydrogen runs out, at first it expands into __________. a superg a white dwarf a star similar to our s

MissTica

Answer: a red giant

Explanation:

When a sun-like star having average mass runs out of fuel-hydrogen, its atmosphere expands and the star becomes a red-giant star. The star would leave the main-sequence stage and enter the red-giant stage in which the pressure of the core is high which pushes the atmosphere outwards and thus the star expands. The pressure also leads to fusion of higher nuclei. The end stage of such a star would be formation of a white dwarf. A heavier star becomes a super-giant, goes supernova and forms a neutron star or a black-hole.

5 0

3 years ago

Read 2 more answers

Calculate the mass (in grams) of 250mL of ether at 25 oC. The density of

leonid [27]

Volume=250mL
Density=0.71g/ml

$\boxed{\sf Density=\dfrac{Mass}{Volume}}$

$\\ \sf{:}\implies Mass=Density(Volume)$

$\\ \sf{:}\implies Mass=0.71(250)$

$\\ \sf{:}\implies Mass=177.5g$

6 0

3 years ago

Consider the reaction 4 HCl(g) + O2(g) =2 H2O(g) + 2 Cl2(g) Using the standard thermodynamic data in the tables linked above, ca

ch4aika [34]

Answer:

The equilibrium constant for this reaction at 298.15 K is $2.067\times 10^{13}$ .

Explanation:

The equation used to calculate Gibbs free change is of a reaction is:

$\Delta G^o_{rxn}=\sum [n\times \Delta G^o_f(product)]-\sum [n\times \Delta G^o_f(reactant)]$

The equation for the enthalpy change of the above reaction is:

$\Delta G^o_{rxn}=(2\times \Delta G^o_f_{(H_2O(g))}+2\times G^o_f_{(Cl_2(g))})-(4\times \Delta G^o_f_{(HCl(g))}+1\times G^o_f_{(O_2(g))})$

We are given:

$\Delta G^o_f_{(HCl(g))}=-95.3 kJ/mol\\\Delta G^o_f_{(H_2O(g))}=228.6 kJ/mol$

$\Delta G^o_f_{(O_2(g))}=\Delta G^o_f_{(Cl_2(g))}=0$ (pure element)

Putting values in above equation, we get:

$\Delta G^o_{rxn}=(2\times (-228.6 kJ/mol)+2\times 0 kJ/mol)-(4\times -95.3 kJ/mol+1\times 0 kJ/mol)=-76 kJ/mol$

To calculate the $K_1$ (at 25°C) for given value of Gibbs free energy, we use the relation:

$\Delta G^o=-RT\ln K_1$

where,

$\Delta G^o$ = Gibbs free energy = -76 kJ/mol = -76000 J/mol

(Conversion factor: 1kJ = 1000J)

R = Gas constant = $8.314J/K mol$

T = temperature = 298.15 K[/tex]

$K_1$ = equilibrium constant at 25°C = ?

$-76000 J/mol=-8.314J/K mol\times 298.145 K\ln K_1$

$\ln K_1=\frac{-76000 J/mol}{-8.314J/K mol\times 298.15 K}$

$K_1=2.067\times 10^{13}$

The equilibrium constant for this reaction at 298.15 K is $2.067\times 10^{13}$ .

8 0

3 years ago

What is the atomic mass of an atom that has 6 protons, 6 neutrons, and 6 electrons? A) 6 B) 8 C) + 1 D) 12 E) 18

Oksana_A [137]

<u>Answer:</u> The correct answer is Option D.

<u>Explanation:</u>

Atomic mass of an atom is defined as the sum of number of neutrons and number of protons that are present in an atom. It is represented as 'A'.

Atomic number = Number of protons + Number of neutrons

We are given:

Number of protons = 6

Number of neutrons = 6

Number of electrons = 6

Atomic mass = 6 + 6 = 12

Hence, the correct answer is Option D.

6 0

3 years ago