Both a globe and a flat world map can module features of the earth. Give an example of when you would use each of these modules.

Given the atomic mass of select elements, calculate the molar mass of each salt. Element Molar mass (g/mol) Beryllium (Be) 9.012

jeka94

Answer:

1. 266.22 g/mol

2. 168.81 g/mol

3. 223.35 g/mol

4. 199.88 g/mol

Explanation:

For you to calculate the molar mass of the salt you need to sum the molar masses of every element in the salt.

In the first salt, PdBr $2_{123}$ , the subscript 2 means that there are 2 atoms of Br. So for you to calculate the molar mass of the salt you need to sum the molar mass of Pd and 2 times the molar mass of Br, as follows:

106 g/mol + 2(79.90 g/mol) = 266.22 g/mol

In the second salt BeBr $2_{123}$ there are 2 atoms of Br and 1 of Be, so the molar mass is:

9.012 g/mol +2(79.90 g/mol) = 186.22 g/mol

In the third salt CuBr $2_{123}$ there are 2 atoms of Br and 1 of Cu, so the molar mass is:

63.55 g/mol + 2(79.90 g/mol) = 223.35 g/mol

And in the fourth salt CaBr $2_{123}$ there are 2 atoms of Br and 1 of Ca, so the molar mass is:

40.08 g/mol + 2(79.90 g/mol) = 199.88 g/mol

6 0

3 years ago

A 30-0 g sample of water at 280 K is mixed with 50.0 g of water at 330 K. How would you calculate the final temperature of the m

aliya0001 [1]

Answer:

311.25k

Explanation:

The question assumes heat is not lost to the surroundings, therefore

heat emitted from hotter sample ( $q_{\ lost}$ )= heat absorbed by the less hotter sample( $q_{\ gain}$ )

The relationship between heat (q), mass (m) and temperature (t) is $q = mc\Delta t$

where c is specific heat capacity, $\Delta t$ temperature change.

$\Delta t$ = $t_{\ final} - t_{\ initial}$

equating both heat emitted and absorb

$-q_{\ lost} = q_{\ gain}$

$-m_{1}(t_{\ final} - t_{\ 1initial})=m_{2}(t_{\ final} - t_{\ 2initial})$

where the values with subset 1 are the values of the hotter sample of water and the values with subset 2 are the values of the less hot sample of water.

C will cancel out since both are water and they have the same specific heat capacity.

so we have

$-m_{1}(t_{\ final} - t_{\ 1initial})=m_{2}(t_{\ final} - t_{\ 2initial})$

where m1 = 50g, t 1initial = 330, m2 = 30g, t2 initial = 280,t final (final temperature of the mixture) = ?

-50 * ( $t_{final}$ - 330) = 30 * ( $t_{final}$ - 280)

-50 $t_{final}$ + 16500 = 30 $t_{final}$ - 8400

80 $t_{final}$ = 16500+8400

80 $t_{final}$ = 24900

$t_{final}$ = 24900/80 = 311.25k

8 0

3 years ago

Find the independent variable and the dependent variable :)))

Naddik [55]

Answer:

dependent variable: plant growth

independent: sunlight impact/amount of light

Explanation:

6 0

4 years ago

How many grams of water are produced from the combustion of 45.2 g of

Zina [86]

Answer:

101.56 of H₂O

Explanation:

The balanced equation for the reaction is given below:

CH₄ + 2O₂ —> CO₂ + 2H₂O

Next, we shall determine the mass of CH₄ that reacted and the mass of H₂O produced from the balanced equation. This is illustrated below:

Molar mass of CH₄ = 12 + (4×1.01)

= 12 + 4.04

= 16.04 g/mol

Mass of CH₄ from the balanced equation = 1 × 16.04 = 16.04 g

Molar mass of H₂O = (2×1.01) + 16

= 2.02 + 16

= 18.02 g/mol

Mass of H₂O from the balanced equation = 2 × 18.02 = 36.04g

SUMMARY:

From the balanced equation above,

16.04 g of CH₄ reacted to produce 36.04 g of H₂O.

Finally, we shall determine the mass of water, H₂O produced by the reaction of 45.2 g of methane, CH₄. This can be obtained as illustrated below:

From the balanced equation above,

16.04 g of CH₄ reacted to produce 36.04 g of H₂O.

Therefore 45.2 g of CH₄ will react to produce = (45.2 × 36.04)/16.04 = 101.56 g of H₂O.

Thus, 101.56 of H₂O were obtained.

7 0

3 years ago

Help?!?! Compare and contrast ionic and covalent compounds

Gnom [1K]

Onic compounds are formed from strong electrostatic interactions between ions, which result in higher melting points and electrical conductivity compared to covalent compounds. Covalent compounds havebonds where electrons are shared between atoms.

7 0

3 years ago