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3 years ago

Dessert biomes have all of these EXCEPT-

1 answer:

7 0

Answer: B). little wind

Explanation: Deserts have few large animals, fertile soil, and little rainfall but they have lots of wind

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Amplitude measures the light's

charle [14.2K]

Answer:

d.) intensity

Explanation:

8 0

3 years ago

Read 2 more answers

Calorimeter containing 1000 grans of water the initial temperature of water is 24.85 degrees . the heat of water is 4.184 j/g de

kvasek [131]

<h3><u>Answer;</u></h3>

10.80 ° C

<h3><u>Explanation;</u></h3>

From the information given;

Initial temperature of water = 24.85°C

Final temperature of water = 35.65°C

Mass of water = 1000 g

The specific heat of water ,c = 4.184 J/g °C.

The heat capacity of the calorimeter = 695 J/ °C

Change in temperature ΔT = 35.65°C - 24.85°C

= 10.80°C

3 0

3 years ago

Various members of a class of compounds, alkenes, react with hydrogen to produce a corresponding alkane. Termed hydrogenation, t

Vitek1552 [10]

<u>Answer:</u> The mass of decane produced is $1.743\times 10^2g$

<u>Explanation:</u>

To calculate the number of moles, we use the equation:

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

Mass of hydrogen gas = 2.45 g

Molar mass of hydrogen gas = 2 g/mol

Putting values in equation 1:, we get:

$\text{Moles of }H_2=\frac{2.45g}{2g/mol}=1.225mol$

The chemical equation for the hydrogenation of decene follows:

$C_{10}H_{20}(l)+H_2(g)\rightarrow C_{10}H_{22}(s)$

As, decene is present in excess. So, it is considered as an excess reagent.

Thus, hydrogen gas is a limiting reagent because it limits the formation of products.

By Stoichiometry of the reaction:

1 mole of hydrogen gas produces 1 mole of decane.

So, 1.225 moles of hydrogen gas will produce = $\frac{1}{1}\times 1.225=1.225mol$ of decane

Now, calculating the mass of decane by using equation 1, we get:

Moles of decane = 1.225 mol

Molar mass of decane = 142.30 g/mol

Putting values in equation 1, we get:

$1.225mol=\frac{\text{Mass of decane}}{142.30g/mol}\\\\\text{Mass of carbon dioxide}=(1.225mol\times 142.30g/mol)=174.3g=1.743\times 10^2g$

Hence, the mass of decane produced is $1.743\times 10^2g$

5 0

3 years ago

How many moles of each reactant are needed to produce 3.60 x 10^2g ch3oh

zysi [14]

Methanol is prepared by reacting Carbon monoxide and Hydrogen gas,

CO + 2 H₂   → CH₃OH

Calculating Moles of CO:
According to equation,

32 g (1 mole) of CH₃OH is produced by = 1 Mole of CO
So,
3.60 × 10² g of CH₃OH is produced by = X Moles of CO

Solving for X,
X = (3.60 × 10² g × 1 Mole) ÷ 32 g

X = 11.25 Moles of CO

Calculating Moles of H₂:
According to equation,

32 g (1 mole) of CH₃OH is produced by = 2 Mole of H₂
So,
3.60 × 10² g of CH₃OH is produced by = X Moles of H₂

Solving for X,
X = (3.60 × 10² g × 2 Mole) ÷ 32 g

X =  22.5 Moles of H₂

Result:
  3.60 × 10² g of CH₃OH is produced by reacting 11.25 Moles of CO and 22.5 Moles of H₂.

3 0

3 years ago

How are Celsius, Kelvin, and Fahrenheit scales similar? How are they different? Considering their differences, think of one scen

PIT_PIT [208]

Answer:

they are similar becauze they measure temperature

6 0

3 years ago