The mass of water in a single popcorn kernel was found to be 0.535 grams after it popped at a temperature of 175 °C. Using the information given in the Introduction, calculate the amount of heat in kilojoules required to pop this single kernel if the room temperature was recorded to be 21.0 °C.
The mass of water in a single popcorn kernel was found to be 0.535 grams after it popped at a temperature of 175 °C. Using the information given in the Introduction, calculate the amount of heat in kilojoules required to pop this single kernel if the room temperature was recorded to be 21.0 °C.
The mass of water in a single popcorn kernel was found to be 0.535 grams after it popped at a temperature of 175 °C. Using the information given in the Introduction, calculate the amount of heat in kilojoules required to pop this single kernel if the room temperature was recorded to be 21.0 °C.
The mass of water in a single popcorn kernel was found to be 0.535 grams after it popped at a temperature of 175 °C. Using the information given in the Introduction, calculate the amount of heat in kilojoules required to pop this single kernel if the room temperature was recorded to be 21.0 °C.
Once we know how much water was inside of the popcorn kernels, we can calculate the temperature at which the kernels popped using the Ideal Gas Law (equation 1), where P is 135 PSI, V is the average volume of a single popcorn kernel, n is the number of moles of water in a single popcorn kernel, and R is the gas constant 0.08206 L atm mol-1 K-1. In order to utilize the Ideal Gas Law equation, we will need to utilize the conversion factor 1 atm = 14.696 PSI to convert PSI to atm. The temperature that we calculate can then be used to determine how much heat was needed in order to heat the water and pop the kernels using equation 2, where m is the mass of water in a popcorn kernel, Troom is the temperature of the room, and Tpop is the temperature you calculated where the kernels popped. For equation 2, sliquid = 4.184 J g-1 °C-1, ΔHvap = 40.65 kJ mol-1, and sgas = 1.996 J g-1 °C-1. In order to utilize equation 2, all energy values must be the same, either in joules or kilojoules.
PV=nRT
(Equation 1)
the attached image is equation 2
(Equation 2)
Transcribed Image Text:**Active Transport: ATP Synthesis Mechanism of Na/K Pump**
**Active Transport**
Active transport is a process that requires energy to move substances across cell membranes. This energy is provided by ATP (adenosine triphosphate). Unlike passive transport, active transport works against the concentration gradient, meaning that it moves substances from an area of low concentration to an area of high concentration.
**Process of Primary Active Transport**
1. **Initial State**: The pump is open towards the inside of the cell, with high affinity for sodium ions.
2. **Sodium Binding**: Three sodium ions inside the cell bind to the pump.
3. **Phosphorylation**: ATP is utilized, and the pump gets phosphorylated. This changes the pump’s shape, opening it to the outside.
4. **Sodium Release, Potassium Binding**: Sodium ions are released outside. The pump now has high affinity for potassium ions, and two potassium ions bind.
5. **Dephosphorylation**: The pump loses phosphate, reverting to its original shape, and opens to the inside of the cell.
6. **Potassium Release**: Potassium ions are released into the cell.
**Diagram Explanation**
- The diagram illustrates the six steps involved in the working of the Na/K pump during active transport.
- Each step is depicted with arrows and labels indicating the specific actions occurring, such as ion binding, ATP utilization, phosphorylation, and shape changes of the transport protein.
Active transport through the Na/K pump is crucial in maintaining the electrochemical gradients across the cell membrane, which is essential for various cellular processes.
Definition Definition Any of various laws that describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. At a constant temperature, the pressure of a particular amount of gas is inversely proportional with its volume (Boyle's Law) In a closed system with constant pressure, the volume of an ideal gas is in direct relation with its temperature (Charles's Law) At a constant volume, the pressure of a gas is in direct relation to its temperature (Gay-Lussac's Law) If the volume of all gases are equal and under the a similar temperature and pressure, then they contain an equal number of molecules (Avogadro's Law) The state of a particular amount of gas can be determined by its pressure, volume and temperature (Ideal Gas law)
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