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3 years ago

List the common ion(s) for tungsten

2 answers:

7 0

. Tungsten is commonly used in heavy metal alloys such as high speed steel, from which cutting tools are manufactured. It is also used in the so-called 'superalloys' to form wear-resistant coatings.

Hope this helps please make my answer brainliest

frozen [14]3 years ago

6 0

What? Uhm tungsten kkkk

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If the reaction of 3.50 moles of lithium with excess hydrofluoric acid produced a 75.5% yield of hydrogen gas, what was the actu

melomori [17]

<u>Answer: </u>The correct answer is 1.32 mol $H_2$

<u>Explanation:</u>

For the reaction of lithium and hydrofluoric acid, the equation follows:

$2Li+2HF\rightarrow 2LiF+H_2$

By Stoichiometry of the reaction:

if 2 moles of lithium is producing 1 mole of hydrogen gas,

Then, 3.50 moles of lithium will produce = $\frac{1}{2}\times 3.5=1.75mol$ of hydrogen gas.

Now, to know the theoretical yield of hydrogen gas, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ ...(1)

Moles of hydrogen gas = 1.75 mol

Molar mass of hydrogen gas = 2 g/mol

Putting values in above equation, we get:

$1.75mol=\frac{\text{Mass of hydrogen gas}}{2g/mol}\\\\\text{Given mass of hydrogen gas}=3.5gl$

To calculate the percentage yield, we use the equation:

$\%\text{ yield}=\frac{\text{Actual yield}}{\text{Theoretical yield}}\times 100$

Percentage yield = 75.5 %

Theoretical yield = 3.5 g

Putting values in above equation, we get:

$75.5=\frac{\text{actual yield}}{3.5g}\times 100\\\\\text{Actual yield}=2.64g$

Now, calculating the moles of hydrogen gas, we put the value in equation 1, we get:

$\text{Moles of hydrogen gas produced}=\frac{2.64g}{2g/mol}=1.32mol$

Hence, the correct answer is 1.32 mol $H_2$

5 0

3 years ago

Read 2 more answers

A 17.98-g piece of iron absorbs 2056.5 joules of heat energy, and its temperature changes from 25°C to 200°C. Calculate the spec

V125BC [204]

Answer: $0.65\ J/g.^{\circ}C$

Explanation:

Given

Mass of iron piece is $m=17.98\ g$

Heat absorbed $Q=2056.5\ J$

Temperature changes from $25^{\circ}C\ to\ 200^{\circ}C$ i.e.

$\Delta T=200-25=175^{\circ}C$

Heat absorbed is given by $Q=mc\Delta T\quad [c=\text{specific heat of material}]$

Insert the values

$\Rightarrow 2056.5=17.98\times c\times 175\\\\\Rightarrow c=\dfrac{2056.5}{3146.5}\\\\\Rightarrow c=0.65\ J/g.^{\circ}C$

Thus, the specific heat of iron is $0.65\ J/g.^{\circ}C$

7 0

3 years ago

Based on the information in the tables, what is the Enthalpy of the solution for each substance? Please help me with this proble

3241004551 [841]

Answer: mg(OH)2 = +37

Rbl = 31

RbOH= -83

mgl2= -144

Explanation: just did it on edge2020

5 0

3 years ago

3. What is the mass of 5 moles of Hydrogen sulfate?I

solong [7]

Answer:

490

98 for 1 mole, Hence for 5 moles 5 X 98 =490.

Explanation:

Brainliest please?

3 0

3 years ago

A student wonders whether a piece of jewelry is made of pure silver. She determines that its mass is 3.25 g. Then she drops it i

nydimaria [60]

Answer:

The jewelry is 2896.54_Kg/m^3 less dense than pure silver

Explanation:

Density of jewellery = (mass of jewellery) ÷ (volume of jewellery)

=3.25g ÷ 0.428mL = 0.00325Kg÷0.000000428m^3 = 7583.46Kg/m^3

The density of silver is 10490_Kg/m^3 which is (10490 - 7583.46) 2896.54_Kg/m^3 more dense than the jewellery

The density of Silver [Ag]

The weight of Silver per cubic centimeter is 10.49 grams or the weight of silver per cubic meter is 10490 kilograms, that is the density of silver is 10490 kg/m³; at 20°C (68°F or 293.15K) at a pressure of one atmospheres.

7 0

3 years ago