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Tanya [424]
3 years ago
6

Which structural adaptation would help a plant survive better in a shady environment?

Chemistry
1 answer:
Gekata [30.6K]3 years ago
3 0

Answer:C.

large leaves

Explanation: I took the test

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6th grade help me pleaseeeee
Vesnalui [34]

Answer:

the answer would be A. cells

Explanation:

just trust me Im a 8th grader and I did that before

7 0
3 years ago
Tertiary or top consumers are animals at the top of the food web. They may feed off either primary or secondary consumers. What
babymother [125]

Answer:

Coyotes, Bald Eagles, & Gray wolf.

7 0
3 years ago
15. A pipe leaks water at a rate of 1.24 mL/s. What is the rate of the water leak in L/hr?<br> ALL
alex41 [277]

Answer:

4.46

Explanation:

1.24 ml= 0.00124 L

3600 s=1 hr

0.00124 x 3600=4.46

8 0
3 years ago
The diagram below shows the layers in Earth's interior.
Arada [10]

Answer:

layer B is liquid because of the inner members and layer A is solid because of the outer members

5 0
2 years ago
A 35.6 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, according to the following reaction. If the temperature ros
Oksana_A [137]
<h3>Answer:</h3>

A) -1.24 × 10^3 kJ/Mol

<h3>Explanation:</h3>

we are given;

Mass of ethanol, m = 35.6 g

Temperature change, Δt(35.0 to 76.0°C) = 41 °C

Specific heat capacity of the calorimeter, c = 23.3 kJ/°C

Molar mass of ethanol = 46.07 g/mol

We are required to the heat change of the reaction.

  • We need to note that the reaction is an exothermic reaction since there is an increase in temperature which means heat was lost to the surroundings.

Therefore; we are going to use the following steps;

<h3>Step 1 : Moles of ethanol </h3>

We know, Moles = Mass ÷ molar mass

Thus, moles of ethanol = 35.6 g ÷ 46.07 g/mol

                                      = 0.773 moles

<h3>Step 2: Enthalpy change or heat change for the reaction.</h3>

Heat change = -mcΔt

but we are given s[pecific heat capacity in Kj/°C and we require heat change in kJ/mol

Therefore;

Heat change = -(cΔt) ÷ n ( n is the number of moles)

                      = -( 23.3 kJ/°C × 41°C) ÷0.773 mol

                    = - 1.24 × 10^3 kJ/Mol

Therefore, values of ΔH of the reaction is -1.24 × 10^3 kJ/Mol

7 0
3 years ago
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